Topic 1 - Key Concepts in Chemistry COMPLETE PK Flashcards
(352 cards)
1
Q
What are the symbol states and what do they stand for?
A
(s)- solid (l)- liquid (g)- gas (aq)- aqueous: dissolved in water
2
Q
What are diatomic molecules?
A
Molecules that only contain two atoms
3
Q
Name the formulae of the following ions: 1. ammonium 2. nitrate 3. sulfate 4. hydroxide 5. carbonate
A
- NH4+ 2. NO3- 3. SO42- 4. OH- 5. CO32-
4
Q
Name the chemical formulae of the following molecules: 1. water 2. ammonia 3. carbon dioxide 4. hydrogen 5. chlorine 6. oxygen
A
- H2O 2. NH3 3. CO2 4. H2 5. Cl2 6. O2
5
Q
How can you write an ionic equation?
A
- Write out the full balanced chemical equation. 2. Split any aqueous substances into their two separate ions. 3. Cross out any ions that are the same on both sides. 4. Write out anything that is left.
6
Q
What is a hazard?
A
Anything that has the potential to cause harm or damage.
7
Q
What is a risk?
A
The risk associated to a hazard is the probability of someone (or something) being harmed if they are exposed to the hazard.
8
Q
What is an oxidising agent and what is its hazard symbol?
A
An oxidising agent provides oxygen which allows other materials to burn more fiercely e.g. liquid oxygen.
9
Q
What is a harmful substance and what is its hazard symbol?
A
A harmful substance is a substance that can cause irritation and reddening and blistering of the skin e.g. bleach. The hazard symbol could be either an exclamation mark inside a rotated red square or a black cross inside an orange square.
10
Q
What is an environmental hazard and what is its hazard symbol?
A
Any substance that is harmful to organisms and to the environment e.g. mercury.
11
Q
What is a highly flammable substance and what is its hazard symbol?
A
A highly flammable substance is a substance that catches fire very easily e.g. petrol. The hazard symbol is a flame inside a red square that has been rotated.
12
Q
What is a toxic substance and what is its hazard symbol?
A
A toxic substance is a substance that can cause death by being consumed in any way (swallowing - breathing in - absorption through skin etc.) e.g. hydrogen cyanide. The hazard symbol is a skull and cross bones inside a rotated red square.
13
Q
What is a corrosive substance?
A
A substance that destroys materials - including living tissues (eyes & skin etc.) e.g. concentrated sulfuric acid.
14
Q
What is a risk assessment?
A
It is a procedure that involves identifying all the hazards posed within a chemical experiment and what the risk is from each hazard; this includes working out how likely it is that something will go wrong and how serious it would be if it did. After this you must think of ways to reduce the risks.
15
Q
Why are hazard symbols used?
A
They are used to indicate the dangers associated with the contents of the container and inform people about safe-working precautions with these substances in the laboratory.
16
Q
How did John Dalton describe atoms at the start of the 19th century?
A
He described atoms as solid spheres and said that different spheres made up the different elements.
17
Q
How did J J Thompson change this model?
A
From his experiments of charge and mass he concluded that atoms must contain smaller - negatively charged particles - electrons. He proposed the ‘plum pudding’ model.
18
Q
How did Ernest Rutherford disprove the ‘plum pudding’ model?
A
In 1909 he conducted the gold foil experiment. They fired positively charged alpha particles at an extremely thin sheet of gold. Some passed through - some were slightly deflected but others were deflected backwards which meant that the positive charge of each atom could not be spread out as the ‘plum pudding’ model described. Rutherford proposed the theory of a nuclear atom: a tiny - positively charged nucleus surrounded by a ‘cloud’ of negative electrons.
19
Q
What is the Bohr model?
A
Niels Bohr realised that electrons in a ‘cloud’ would be attracted to the nucleus - causing the atom to collapse so he proposed a new model where the electrons were contained in shells. he said that electrons can only exist in fixed shells which must have a fixed energy.
20
Q
What is the current model of an atom?
A
It is a nucleus containing protons and neutrons surrounded by electrons in shells.
21
Q
Describe the nucleus.
A
It contains protons and neutrons and is in the middle of an atom. It has a positive charge due to the protons and compared to the overall size of the atom - the nucleus is very small - so the mass of an atom is concentrated in the nucleus as electrons have hardly any mass.
22
Q
Describe electrons.
A
They orbit the nucleus in electron shells (or energy levels) and have a negative charge (-1.) Although - they are very small - their orbits cover a large space and each electron has a negligible weight (roughly equal to 1/1835.)
23
Q
Describe protons.
A
They are positively charged (+1) and are contained within the nucleus. They have a mass of 1.
24
Q
Describe neutrons.
A
They are contained within the nucleus and do not have a relative charge. They have a relative mass of 1.
25
Why do atoms have the same number of protons and electrons?
Atoms are neutral so do not have a charge therefore they have the same number of electrons and protons as they are oppositely charged (-1 and +1 respectively.) The charges cancel each other to give 0.
26
What is the atomic number of an atom?
It is the number of protons (and therefore electrons) within an atom.
27
What is the mass number of an atom?
It gives the total number of protons and neutrons in an atom.
28
What are isotopes of an element?
They are different atoms of the same element that contain the same number of protons (as this is unique to the element) but a different number of neutrons in their nuclei so they have a different mass number.
29
What is the relative atomic mass (Ar) of an element?
It is the average mass of one atom of there element compared to 1/12 of the mass of one atom of carbon-12.
30
Why might the Ar of an element be a decimal?
If the element exists as more than one isotope, Ar is an average of the masses, considering how common they are.
31
How can Ar be worked out from isotopic abundances?
1. Multiply each relative isotopic mass by its isotopic abundance 2. Add the results 3. Divide by the total of the abundances (100 if in percentages)
32
How did Dmitri Mendeleev the 50 or so known elements at the time (1868)?
Arranged into the Table of Elements by sorting them into groups based on properties of them and their compounds; realised that if put in order of atomic mass a pattern appeared- he could put elements with similar properties into columns.
33
What were the problems with Mendeleev's arrangement of the elements?
Some elements ended up in the wrong columns and some's atomic mass was wrong due to isotopes. Some because they didn't fit pattern; he switched order to keep elements with similar properties in same columns.
34
What did Mendeleev also have to do to keep elements with similar properties together?
He had to leave gaps; he used properties of elements in same column to predict their properties; when they were found﹐ they fitted pattern; e.g. Mendeleev predicted chemical and physical properties of element called ekasilicon﹐ which we know today as germanium.
35
How is the periodic table arranged today?
1. In order of atomic number rather than atomic mass once protons and electrons were discovered; fit same pattern that Mendeleev worked out 2. Columns called groups and have elements with similar chemical properties 3. Group number = number of electrons in outer shell; group 8 or 0 has full outer shell 4. Rows called periods and each one represents another full shell of electrons; period element is in = number of electron shells it has.
36
What are electron shells also known as?
Energy levels
37
How many electrons can be allowed in each shell?
1. 2 2. 8 3. 8 4. 18
38
What are ions?
Charged particles- can be single atoms or groups of atoms
39
Why might atoms become ions?
They lose or gain electrons to have a full outer shell and so a stable electronic structure; usually metals.
40
What are anions?
Negative ions that form when atoms gain electrons; non-metals.
41
What are cations?
Positive ions that form when atoms lose electrons.
42
Which elements are the most likely to form ions?
Those in groups 1﹐ 2﹐ 6 and 7.
43
What are the three types of bonding?
1. Ionic 2. Metallic 3. Covalent
44
What happens when a metal and a non-metal react with each other?
The metal atom loses electrons to form positive cation; non-metal gains these electrons to form negative anion; oppositely charged ions are strongly attracted to one another by electrostatic forces so bond ionically.
45
How can the arrangement of electrons in an atom or ion be shown?
Dot and cross diagram
46
How can you draw a dot and cross diagram for an ionic compound?
Use dots for electrons of one atom﹐ and crosses for the other; draw all electron shells and electrons and transfer electrons that are lost and gained; draw square brackets around ions in compound and write charge in top right corner.
47
What is the structure of ionic compounds?
A giant ionic lattice; ions form closely packed regular lattice; there are very strong electrostatic forces of attraction between oppositely charged ions in all directions.
48
What are the properties of ionic compounds?
1. High melting and boiling points as large amount of energy needed to overcome strong attraction between ions 2. Don't conduct electricity when solid as ions in fixed place and can't move; when molten﹐ ions free to move and will carry an electric current 3. Dissolve easily in water- ions separate and move freely in solution so will carry an electric current
49
What are the advantages and disadvantages of 2D representations of molecules?
A. Simple; great at showing atoms the molecule contains and how atoms connected D. Don't show shape of substance﹐ and don't give indication of size of atoms
50
What are the advantages and disadvantages of dot and cross diagrams?
A. Useful for showing how compounds or molecules formed and where electrons in the bonds or ions came from D. Don't usually show anything about size of atoms/ions or how they're arranged
51
What are the advantages and disadvantages of 3D models of ionic solids?
A. Show arrangement of ions D. Only show outer layer of substance
52
What are the advantages and disadvantages of ball and stick models?
A. Help to visualise structure and show shape of lattice or molecule in 3D; more realistic than 2D drawings D. Misleading- make it look like there are big gaps between atoms but this is where electron clouds interact; don't show correct scales of atoms/ions which are really different sizes.
53
What is a covalent bond?
A strong bond that forms when a pair of electrons is shared between two atoms; simple molecular substances are made up of molecules containing few atoms joined by covalent bonds.
54
Give some examples of simple molecular substances.
1. Hydrogen﹐ H subscript 2 2. Hydrogen chloride﹐ HCl 3. Water﹐ H subscript 2 O 4. Oxygen﹐ O subscript 2 5. Methane﹐ CH subscript 6. Carbon dioxide﹐ CO subscript 2
55
How big are simple molecules generally?
10 superscript -10 m.
56
What is specific to the dot and cross diagrams of simple molecular substances?
They only show the electrons in the outer shell of each atom.
57
What are the properties of simple molecular substances?
1. Usually have simple molecular structures 2. Atoms held together by very strong covalent bonds (intramolecular forces)﹐ whereas intermolecular forces between these molecules are very weak 3. Low melting and boiling points as little energy needed to break feeble intermolecular forces 4. Most are gases/liquids at room temperature 5. As molecules get bigger﹐ intermolecular forces get stronger to melting and boiling points increase 6. Don't conduct electricity as don't contain any free electrons or ions 7. Some soluble﹐ some aren't
58
What are polymers?
Molecules made up of long chains of covalently bonded carbon atoms; formed when lots of small molecules called monomers join together.
59
Describe the structure of giant covalent molecules.
All the atoms are bonded to each other by strong covalent bonds.
60
Describe the properties of giant covalent structures.
1. Very high melting points as lots of energy needed to break covalent bonds 2. Generally don't conduct electricity as they don't contain charged particles (except graphite and graphene) 3. Not soluble in water
61
Give some examples of carbon-based giant covalent structures.
1. Diamond 2. Graphite 3. Graphene
62
Describe the properties of diamond.
1. Made up of network of carbon atoms﹐ each forming four covalent bonds 2. High melting point as lots of energy needed to break strong covalent bonds 3. Really hard as strong covalent bonds hold atoms in rigid lattice structure- used to strengthen cutting tools 4. Doesn't conduct electricity as no free electrons/ions
63
Describe the properties of graphite.
1. Each carbon atom form three covalent bonds﹐ creating sheets of carbon atoms arranged in hexagons 2. No covalent bonds between layers﹐ only held together weakly so are free to move over each other- graphite soft and slippery used as lubricant 3. High melting point- due to strong covalent bonds 4. Conducts electricity as only three of each carbon's outer four electrons are used in bonds so each atom has one delocalised electron that can move and carry a charge
64
Describe the properties of graphene.
1. One layer of graphite- a type of fullerene 2. Sheet of carbon atoms joined in hexagons 3. Just one atom thick so a 2-dimensional compound
65
What are fullerenes?
Molecules of carbon﹐ shaped like closed tubes or hollow balls; mainly made of carbon atoms arranged in hexagons﹐ but can also be pentagons or heptagons.
66
Describe some uses of fullerenes.
1. Can be used to cage other molecules﹐ trapping it inside- so could be used to deliver drug directly to cells in the body 2. Huge surface area so could make great industrial catalysts- individual catalyst molecules could be attached to fullerene
67
Describe the properties of buckminsterfullerene.
1. Molecular formula = C subscript 60 2. Forms hollow sphere; made up of 20 hexagons and 12 pentagons. 3. Stable molecule that forms soft brownish-black crystals
68
Describe nanotubes (a type of fullerene).
1. Tiny cylinders of graphene- so conduct electricity 2. High tensile strength so can be used to strengthen materials without adding much weight e.g. strengthen sports equipment that needs to be strong and lightweight i.e. tennis rackets
69
Describe metallic bonding.
1. Metals consist of giant structure 2. Electrons in outer shell of metal atoms are delocalised 3. Strong forces of electrostatic attraction between positive metal ions and shared negative electrons 4. Used to hold together compounds of metallic elements and alloys
70
Why is metallic bonding very strong?
Electrostatic forces between metal ions and delocalised sea of electrons are very strong﹐ so need lots of energy to be broken.
71
Describe the physical properties of metals.
1. Most compounds with metallic bonds have very high melting and boiling points due to structure so are usually shiny solids at room temperature 2. Not soluble in water 3. Generally more dense than non-metals as ions in metallic structure are packed closer together 4. Layers of atoms in pure metal can slide over each other﹐ making metals malleable- can be hammered or rolled into flat sheets 5. Delocalised electrons carry electrical current and thermal energy through material so they're good conductors of electricity and heat
72
What is the conservation of mass?
During a chemical reaction﹐ no atoms are destroyed or created so there are the same number and types of atoms on each side of the equation and the total mass is conserved.
73
If a reaction causes a loss or gain of mass﹐ what can be deduced?
It is not a closed system.
74
Why might the mass seem to increase in an unsealed reaction vessel?
1. Probably because at least one of products is a gas found in air and the products are solids﹐ liquids or aqueous 2. Before reaction﹐ gas is floating around in the air; it's there but not contained in reaction vessel so its mass can't be measured 3. When gas reacts to form part of product﹐ it becomes contained inside reaction vessel 4. So total mass inside vessel increases
75
Why might the mass seem to decrease in an unsealed reaction vessel?
1. Probably because some or all of reactants are solids﹐ liquids or aqueous and at least one of the products is a gas 2. Before reaction﹐ all reactants contained in vessel so mass can be measured 3. If vessel isn't enclosed﹐ gas can escape as it's formed so its mass can't be measured 4. Total mass inside vessel decreases
76
How can you work out the relative formula mass﹐ M subscript r﹐ of a compound?
Add the relative atomic masses﹐ A subscript r﹐ of all of the atoms within its formula.
77
What is the empirical formula of a compound?
The simplest whole number ratio of the atoms within the compound.
78
What is a mole?
An amount of particles (e.g. atoms﹐ molecules or ions) that is equal to Avogadro's constant: 6.02 x 1023
79
How is the number of moles related to the mass of a substance?
One mole of atoms or molecules of any substance will have a mass in grams equal to the relative particle mass (A or M subscript r) for that substance.
80
What is the formula for working out the number of moles of a substance?
Moles = mass in grams (of element or compound)/ M or A subscript r of a compound or of an element
81
What is the concentration of a solution?
How crowded the particles are in the solution.
82
How can you convert cm cubed into dm cubed?
Divide by 1000
83
How can you calculate the empirical formula of a compound from the masses of the elements it contains?
1. Work out how many moles of each element there are. 2. Put the number of moles into a ratio and simplify it as far as possible.
84
How could you use an experiment to find empirical formulae?
1. Get crucible and heat until red hot to clean it from previous experiment 2. Leave to cool﹐ weight it﹐ along with its lid 3. Add magnesium ribbon and reweigh with crucible﹐ magnesium and lid 4. Magnesium mass is second mass minus the first mass 5. Heat crucible containing magnesium; put lid on to stop solid from escaping but leave gap to allow oxygen into crucible 6. Heat strongly for around 10 minutes or until ribbon has turned white 7. Allow to cool and reweigh crucible with lid and contents 8. Mass of magnesium oxide is this reading minus initial reading for crucible and lid.
85
How can empirical formulae be worked out from the magnesium ribbon experiment?
1. Work out mass of oxygen as difference between mass of magnesium and magnesium oxide 2. Work out number of moles of magnesium and oxygen atoms involved 3. Divide both values by the lowest result to obtain the simplest ratio
86
What is a limiting reactant?
Reactant that is completely used up in a reaction - stopping the reaction.
87
How can the non-limiting reactants be described?
They are in excess
88
How is the amount of product formed related to the amount of the limited reactant used?
They are directly proportional as long as the other reactants are in excess.
89
The model of atoms has barely changed/changed quite a lot over time
changed quite a lot
90
Rutherford was responsible for discovering...
The nucleus and protons
91
Who discovered neutrons?
Chadwick
92
Who developed the current model of atoms?
Bohr
93
Where are electrons located in an atom?
On the outer shells
94
Where are protons located in an atom?
In the nucleus
95
Where are neutrons located in an atom?
In the nucleus
96
What is the mass of protons?
1
97
What is the charge of protons?
+1
98
What is the mass of neutrons?
1
99
What is the charge of neutrons?
0
100
What is the mass of electrons?
1/2000
101
What is the charge of electrons?
-1
102
The atomic number is the larger/smaller number shown with the element on the periodic table
smaller
103
The mass number is the larger/smaller number shown with the element on the periodic table
larger
104
What does the atomic number tell us?
The number of protons in an atom
105
What does the mass number tell us?
The number of protons + the number of neutrons
106
The number of electrons in an atom is equal to the number of...
protons
107
Protons = which number?
Atomic number
108
Electrons = which number?
Atomic number
109
The number of neutrons in an atom = ...
Mass number - atomic number
110
What is an isotope?
Something that has the same number of protons but a different number of neutrons
111
A proton is what identifies...
The identity of an atom
112
Why do some elements have .5 mass?
The atomic mass is the relative abundance of all isotopes
113
The mas number of Chlorine is 35.5 because...
There are 2 main isotopes of chlorine, chlorine 35 and chlorine 37. 75% of naturally occurring isotopes are chlorine 35 and 25% are chlorine 37.
114
What are the 2 main isotopes of chlorine?
Chlorine 35 and chlorine 37
115
75% of naturally occurring isotopes of chlorine are...
chlorine 35
116
25% of naturally occurring isotopes of chlorine are...
chlorine 37
117
The periodic table is a list of all the ________ which are known to exist
elements
118
Elements are a single type of \_\_\_\_
atom
119
An atom is...
A very small thing
120
When they named atoms they thought they were the...
smallest things possible
121
True/False: There are still lots of elements yet to be discovered
True
122
What is a compound?
2 or more elements that are chemically bonded together
123
Who was the first attempt at a periodic table by?
Newland
124
What did Newland try to do when making the first periodic table?
Group things into octaves and rate them by pattern
125
What was the problem with Newland's first periodic table, involving iron and oxygen?
They were in the same group - these have very different properties
126
Newland arranged elements in the periodic table by \_\_\_\_
mass
127
True/False: Newland left lots of gaps in his periodic table
False, he left no gaps
128
What did Newland do which meant his periodic table didn't really work?
He tried to force things in to have similar patterns or properties as other things
129
Mendeleev's periodic table came before/after Newland
after
130
How did Mendeleev arrange elements in his periodic table?
By mass
131
What did Mendeleev do in his periodic table which Newland hadn't done?
Left gaps
132
In Mendeleev's periodic table, he arranged things in groups with...
Similar patterns
133
Because Mendeleev left gaps in his periodic table and arranged things in groups with similar patterns, he could...
Predict the properties of elements that have yet to be discovered
134
Mendeleev was correct/incorrect with his predictions of elements yet to be discovered
Correct
135
A few years after Mendeleev had developed his periodic table, a couple new elements were discovered and they...
fitted in really neatly to his periodic table
136
After a few new elements were discovered and fitted really neatly in Mendeleev's periodic table, his table was...
accepted
137
How has the periodic table changed since Mendeleev developed his version?
Things are now arranged by electronic arrangement
138
The periodic has changed lots/little in terms of its layout since Mendeleev developed his version
Little
139
Groups go ____ the periodic table
down
140
Periods go ______ the periodic table
across
141
Group 8 is also known as...
Group 0
142
What do groups tell us?
The number of electrons in an atom's outer shell
143
Things in group 2 have _ electrons in their outer shell
2
144
Things in group 6 have _ electrons in their outer shell
6
145
Which two elements are in the first period of the periodic table?
Hydrogen and helium
146
Periods relate to...
the number of shells that things have
147
We can use the information we get from what group and period an element is in to learn about the...
electronic configuration
148
Magnesium's atomic number is 12, therefore magnesium has __ electrons
12
149
Magnesium is in group 2, therefore it has _ electrons on the outer shell
2
150
Magnesium is in period 3, therefore it has _ shells
3
151
How many electrons can fit on the first shell of an atom?
2
152
How many electrons can fit on each shell of an atom, apart from the first one?
8
153
From the fact that there are 2 elements in the first period, we know that the first shell can hold a maximum of _ electrons
2
154
From the fact that there are 8 elements in the second period, we know that the second shell can hold a maximum of _ electrons
8
155
From the fact that there are 8 elements in the third period, we know that the third shell can hold a maximum of _ electrons
8
156
Metals lose/gain electrons
lose
157
When metals lose electrons, they get a positive/negative charge
positive
158
When non-metals gain electrons, they get a positive/negative charge
negative
159
Things in group 1 lose _ electron(s)
1
160
Because things in group 1 lose 1 electron, they become __ ions
+1
161
Things in group 2 lose _ electron(s)
2
162
Because things in group 2 lose 2 electrons, they become __ ions
+2
163
Things in group 7 gain/lose electrons
gain
164
Things in group 2 gain/lose electrons
lose
165
Things in group 6 are metals/non-metals
non-metals
166
Things in group 6 gain _ electron(s)
2
167
Because things in group 6 gain 2 electrons, they become __ ions
-2
168
Things in group 7 gain _ electron(s)
1
169
Because things in group 7 gain an electron, they become __ ions
-1
170
What is ionic bonding?
The transfer of electrons from a metal to a non-metal
171
Ionic bonding is the transfer of electrons from what to what?
A metal to a non-metal
172
Metals can be found on which side of the periodic table?
The left
173
Non-metals can be found on which side of the periodic table?
The right
174
Magnesium being in group 2 tells us that is has...
2 electrons in its outer shell
175
Oxygen being in group 6 tells us that is has...
6 electrons in its outer shell
176
In ionic bonding, would oxygen gain electrons or lose electrons?
Gain
177
Why does oxygen gain electrons in ionic bonding?
It is a non-metal
178
Why are the diagrams used to show ionic bonding called dot and cross diagrams?
One element's electrons are represented with a dot and the other a cross
179
What must we draw around ions after ionic bonding?
Square brackets
180
After we have drawn square brackets around ions, what must we indicate?
The charge of the ions
181
During ionic bonding, magnesium loses two electrons. What is its charge?
+2
182
During ionic bonding, oxygen gains two electrons. What is its charge?
-2
183
Sodium has an atomic number of 11, meaning...
that there will be 11 protons in the nucleus
184
Protons have a ________ charge
positive
185
In an atom, the positive charges and negative charges...
cancel each other out
186
Because the positive and negative charges in an atom cancel each other out, the overall charge of atoms is...
0
187
During ionic bonding, sodium would gain/lose electron(s)
Lose
188
Because sodium loses an electron during ionic bonding, sodium ions have what overall charge?
Positive
189
A +1 sodium ion would have one more...
proton than electron
190
What is the structure of ionic compounds?
A giant ionic lattice
191
Ionic compounds have a high/low melting point
high
192
Ionic compounds have a high/low boiling point
high
193
Ionic compounds only conduct electricity when...
molten or dissolved
194
Why do ionic compounds only conduct electricity when molten or dissolved?
Ions need to be free to move
195
Covalent bonding is the...
sharing of electrons between two non-metals
196
Covalent bonding happens between...
Two non-metals
197
Hydrochloric acid includes...
One element of hydrogen and one element of chlorine
198
What is another name for hydrogen chloride?
Hydrochloric acid
199
What does the formula HCl represent?
Hydrochloric acid / hydrogen chloride
200
How would you represent the covalent bonding of hydrochloric acid with lines?
H-Cl
201
The attached image shows what type of bonding?
Covalent
202
What does this dot and cross diagram show?
The covalent bonding of hydrogen and chlorine to make hydrochloric acid
203
What is the chemical formula for ammonia?
NH3
204
What does the formula NH3 represent?
Ammonia
205
How would you represent the covalent bonding of ammonia with lines?
H - N - H
|
H
206
What does this dot and cross diagram show?
The covalent bonding of nitrogen and hydrogen to make ammonia
207
What is the chemical formula for methane?
CH4
208
How would you represent the covalent bonding of methane with lines?
H
|
H - C - H
|
H
209
What does the formula CH4 represent?
Methane
210
What does this dot and cross diagram show?
The covalent bonding of carbon and hydrogen to make methane
211
What is the chemical formula for hydrogen gas?
H2
212
What does the formula H2 represent?
Hydrogen gas
213
How would you represent the covalent bonding of two hydrogen atoms with lines?
H - H
214
What does this dot and cross diagram show?
The covalent bonding of two hydrogen atoms
215
What is the chemical formula for the covalent bonding of chlorine?
Cl2
216
What does the formula Cl2 represent?
Chlorine gas
217
How would you represent the covalent bonding of chlorine gas with lines?
Cl - Cl
218
What does this dot and cross diagram represent?
The covalent bonding of chlorine gas
219
How would you representthe covalent bonding of two oxygen atoms with lines?
O = O
220
What is the chemical formula for oxygen gas?
O2
221
What is special about oxygen atoms' bond?
They have a double bond
222
What does the formula O2 represent?
Oxygen gas
223
What does this dot and cross diagram represent?
The covalent bonding of oxygen
224
Each line in line drawings of covalent bonding is equal to...
a pair of electrons
225
Why are there 4 electons being shared in the middle?
Oxygen has a double bond
226
Oxygen has a double bond, meaning how many electrons will be shared between atoms?
4
227
Nitrogen has what type of bond?
A triple bond
228
What is the chemical formula for two nitrogen atoms?
N2
229
What does the formula N2 represent?
Two nitrogen atoms
230
How would you represent the covalent bonding of two nitrogen atoms with lines?
N ≡ N
231
What does this dot and cross diagram represent?
The covalent bonding of two nitrogen atoms
232
Why are there 6 electons being shared in the middle?
Nitrogen has a triple bond
233
Nitrogen has a triple bond, meaning how many electrons will be shared between atoms?
6
234
Label the formula
C5H12
235
Label the formula
C3H8O
236
Why is C5H12 incorrect for this formula?
The numbers are written too big
237
Why is C5H12 incorrect for this formula?
The numbers are in the wrong place
238
What is the formula for carbon dioxide?
CO2
239
What is the formula for water?
H2O
240
What is the formula for oxygen gas?
O2
241
What is the formula for hydrogen gas?
H2
242
What is the formula for nitrogen gas?
N2
243
What is the formula for ammonia?
NH3
244
What is the formula for hydrochloric acid?
HCl
245
What is the formula for sulfuric acid?
H2SO4
246
Give 3 examples of simple covalent compounds
Any 3 from H2O, CO2, O2, N2, H2, HCl and CH4
247
Simple covalent compounds are very large/small structures
small
248
Simple covalent compounds have what type of bonding?
Covalent
249
Simple covalent compounds have high/low melting points
low
250
Simple covalent compounds have high/low boiling points
low
251
Simple covalent compounds are generally what at room temperature?
A gas or a liquid
252
Simple covalent compounds do/do not conduct electricity
do not
253
What are graphite and diamond made from?
Carbon
254
Give 3 examples of giant covalent compounds
Any 3 from graphite, diamond, fullerines and silicon dioxide
255
What structure do giant covalent compounds have?
A giant covalent structure
256
Giant covalent compounds have high/low melting points
high
257
Giant covalent compounds have high/low boiling points
high
258
Giant covalent compounds do/do not conduct electricity
do not
259
Giant covalent compounds do/do not dissolve
do not
260
What is the structure of diamond?
giant covalent compound/lattice
261
What is diamond made of?
Pure carbon
262
Each carbon in diamond makes how many bonds?
4
263
Diamond is incredibly soft/hard
hard
264
Diamond is very common/rare
rare
265
Why do we use diamond in drills?
It is incredibly hard
266
What is the structure of graphite?
Giant covalent
267
What is graphite made of?
Pure carbon
268
Each carbon in graphite makes how many bonds?
3
269
Graphite is soft/hard
soft
270
True/False: Graphite does not conduct electricity
False, it does
271
Why does graphite conduct electricity?
It is in sheets and there is a spare electron floating around in between
272
True/False: Graphite is in sheets
True
273
What is between the sheets in graphite that allow electrcity to be conducted?
A spare electron foating around
274
What is a single sheet of graphite called?
Graphene
275
Graphite can be found in...
pencils
276
Graphite and diamond are made of...
pure carbon
277
Graphite is made of how many carbon-carbon bonds?
3
278
Diamond is made out of how many carbon-carbon bonds?
4
279
True/False: Graphite and diamond are both hard
False, graphite is soft, diamond is hard
280
Fullerenes are either...
Carbon nanotubes or buckminsterfullerenes
281
What shape are buckminsterfullerenes?
Balls
282
What shape are carbon nanotubes?
Tubes
283
Carbon nanotubes are made of...
pure carbon
284
Buckminsterfullerenes are made of...
pure carbon
285
Fullerenes make how many carbon-carbon bonds?
3
286
Give 2 examples of fullerenes
Carbon nanotubes and buckminsterfullerenes
287
Carbon nanotubes are very soft/hard
hard
288
Buckminsterfullerenes are very soft/hard
hard
289
Give 2 things that buckminsterfullerenes can be used for
Any 2 from a lubricant, reinforcement and drug delivery
290
Things that need lubricating such as electrical cycles or some parts of machines may use...
buckminsterfullerenes
291
Give an example of how buckminsterfullerenes can be used as reinforcement
When you need a very strong and light thing such as aircraft and bicycles
292
In the future, carbbon nanotubes and buckminsterfullerenes will both be used for...
Drug delivery
293
There are loads of potentials for fullerenes but...
They haven't been realised yet
294
Whether polymers have crosslinks or not determines...
what their properties are going to be like
295
Polymers that have crosslinks are/aren't very fixed in place
are
296
Polymers that have crosslinks will/will not burn upon heating
will
297
Polymers that do not have crosslinks will ____ upon heating
melt
298
Why do polymers that don't have crosslinks melt upon heating?
Because they can slide across each other whereas polymers with crosslinks can't
299
True/False: Polymers with crosslinks can slide across each other
False, they cannot
300
Metals are made up of positive/negative ions in a...
positive, in a sea of delocalised electrons
301
Metals are made up of what in a sea of delocalised electrons?
Positive ions
302
Metals are made up of positive atoms in...
a sea of delocalised electrons
303
Metals are made up of positive atoms in a sea of what?
Delocalised electrons
304
Why can metals conduct electricity?
Their delocalised electrons are free to move
305
The fact that delocalised electrons in metals are free to move means that...
metals can conduct electricity and heat well
306
Why are metals so good at conducting heat?
Their delocalised electrons are free to move
307
An alloy looks the same as/slightly different to a metal
slightly different to
308
True/False: Alloys, like metals, have positive ions and delocalised electrons
True
309
What makes an alloy different from a metal?
Although they both have positive ions and delocalised electrons, there is something else in alloys aswell such as maybe another metal that it has alloyed with or something like carbon
310
Although alloys have positive ions in a sea of delocalised electrons, they also have...
something else metal or non-metal that it has alloyed with in there aswell
311
Give an example of something that an alloy can alloy with
A metal or non-metal, such as carbon
312
What type of metals have layers?
Pure metals
313
What do layers in metals do?
Slide across each other
314
The fact that pure metals have layers that can slide means...
they are soft
315
Do alloys have layers?
They don't have layers or they have distorted layers
316
Distorted layers in alloys can/cannot slide
cannot
317
The fact that alloys have distorted layers that cannot slide means...
they are hard
318
Acid + metal -\>
Salt + hydrogen
319
Acid + metal oxide -\>
Salt + water
320
Acid + metal hydroxide -\>
Salt + water
321
Acid + metal base -\>
Salt + water
322
Acid + metal carbonate -\>
Salt + water + carbon dioxide
323
To work out the forumula of salts, you need to figure out...
the formula of the ions
324
When working out the formula of salts you need to combine ions in such a way that they are...
neutral overall
325
What is the formula for magnesium?
Mg
326
What does the acronym MASH tell us?
Metal + acid -\> salt + hydrogen
327
HCl + Mg -\> MgClx + H2
What is the value of x, and why?
2, because Mg is a +2 ion and Cl is a -1 ion. These need to be balanced so we put the 2 so we have 2 -1 ions, making the overall charge neutral
328
Balance the following equation:
HCl + Mg -\> MgCl2 + H2
2HCl + Mg -\> MgCl2 + H2
329
Water -\> hydrogen + oxygen
What is the unbalanced chemical equation?
H2O -\> H2 + O2
330
Balance the following equation:
H2O -\> H2 + O2
2H2O -\> 2H2 + O2
331
What does Mr mean?
Relative formula mass
332
How do you calculate the relative formula mass of something?
Add all of the relative atomic masses together
333
What does Ar mean?
Relative atomic mass
334
The mass number is the smaller/larger number
larger
335
How would you calculate the relative formula mass of H2SO4?
(2 x the atomic mass of hydrogen) + (1 x the atomic mass of sulfur) + (4 x the atomic mass of oxygen)
336
What does empirical formula mean?
The lowest ratio of all of the elements in a compound
337
If we have an element that is 75% carbon and 25% hydrogen, what is the first step in calculating the empirical formula?
Find the mass of carbon and hydrogen and divide the number in the question by the mass. (75 / 12 and 25 / 1)
338
When calculating empirical formula, what do we do after we have divided the percentages in the question by the masses of the elements in the compound?
Divide the largest number by the smallest number
339
What is the empirical formula for a compound that has 1 carbon atom for every 4 hydrogen atoms?
CH4
340
What is a mole?
The unit for the amount of a substance
6 x 1023
341
True/False: Moles are the unit for the amount of atoms
False, they are the unit for the amount of a substance so although this can be atoms, it can also be ions, molecules, etc
342
Why do we use moles (6 x 1023) as the units for the amount of a substance?
That is the amount of carbon atoms in 12g of carbon
343
The equation for moles is...
moles = mass / Mr
344
Balance the following equation:
H2O2 -\> H2O + O2
2H2O2 -\> 2H2O + O2
345
This is the balanced equation showing that hydrogen peroxide (H2O2) decomposes in to water and oxygen. How would we calculate how much oxygen gas will be given off from 40.8g of hydrogen peroxide?
2H2O2 -\> 2H2O + O2
Find the Mr of each compound by multiplying the mases by the number of each element there in each compound and adding them together. This would give you the ratio of the products. You would then scale this up/down using ratios as you would in maths to find how much would be given off from 40.8g.
346
What is the equation for concentration?
Amount / volume
347
What is concentration measured in?
mol/dm3
348
When calculating concentration, what is the amount of a substance measured in?
mol
349
When calculating concentration, what is the volume measured in?
dm3
350
When you have an equation there is always going to be a limiting...
reactant
351
What is a limiting reactant?
A reaction will continue forming a product until you get to the point where your limiting reactant is used up, at which point the reaction will stop
352
Whatever you don't want your limiting reactant to be, you need to make sure that...
it is in excess
