Unit A Energy and Matter in Chemical Change : Section 2.0 Flashcards
(174 cards)
1
Q
What is the foundation for everything?
A
The elements
2
Q
How many elements are in the periodic table?
A
118
3
Q
What are elements?
A
Substances that cannot be broken down
4
Q
How many naturally occurring elements are there?
A
90
5
Q
How many synthetic elements are there?
A
25
6
Q
What are the three sections that all elements can be classified into?
A
Metals
Non-metals
Metalloids
7
Q
What section do most elements fall into?
A
Metals
8
Q
Which section has the least elements?
A
Metalloids
9
Q
What are the six common characteristics of metalloids?
A
- Silver or gray
- Shiny
- Good conductors
- Malleable
- Ductile
- Solid at room temperature
10
Q
How does mercury differ from other metals?
A
It is a liquid at room temperature
11
Q
What is room temperature?
A
25°
12
Q
What is an example of a variable characteristic of a metal?
A
-How strongly metals react with other substances.
13
Q
Which metal is highly reactive with air and water?
A
Sodium
14
Q
What are some examples of inert metals?
A
Gold and platinum
15
Q
What does inert mean?
A
Unreactive
16
Q
How many elements are non-metals?
A
17
17
Q
Why are non-metals in a section together?
A
Because of their lack of resemblance to metal instead of their similarities
18
Q
What type of bond are about half of the non-metals usually in? What name can we give these compounds?
A
molecular bond / covalent bond;
molecules
19
Q
What type of variation is there in non-metals?
A
There is a lot of variation among non metals, particularly in colour and state. For example many are colorless gases but as liquids can be slightly colored like light blue liquid oxygen. Carbon is black when graphite and clear when diamond. Hydrogen, helium, and nitrogen are clear and colorless when gas or liquid. Sulphur is bright yellow and forms large crystals. Boron is black brown. Phosphorus has many different colours including colorless, waxy white, scarlet, red, violet, yellow, or black. P4 is white. Fluorine is pale yellow as a gas. Iodine appears violet as a gas but is nearly black as a solid (shiny and a hint of purple). Astatine is a black solid.
In contrast, metals are solid and usually silver except for copper, gold, and osmium. Copper is shiny and close in colour to a mix of red, orange and brown, gold is golden, and osmium is silvery blue.
20
Q
What non-metal can etch glass?
A
Flourine
Hydrofluoric acid HFl and potassium fluoride KFl are used commonly
21
Q
Which group on the periodic table is unreactive?
A
Noble gases
22
Q
What are metalloids?
A
Elements that have properties that are intermediate between metals and non-metals
23
Q
What properties does the periodic table organize elements by?
A
Chemical properties
24
Q
Which side of the periodic table are the metals located on?
A
The left
25
Which side of the periodic table are the non-metals located?
The right
26
Where are the metalloids on the periodic table located?
In between the metals and non-metals
Above and below the staircase, not including aluminum, and not including the halogens. Start the staircase to the left and below Boron and go down to the right.
27
Why is hydrogen an exception? (context = metal vs. non-metal)
It is a non-metal but behaves like metal in chemical reactions
28
How does an element get its symbol?
Its often an abbreviation derived from the element's name. Will have at least one uppercase letter. May also have a lower case letter as a second letter.
29
What is a Period?
Each horizontal row, where period 1 is the first row and period 2 is the second row in the periodic table etc.
30
What is a group?
Each vertical coulumn is considered a group; several of the groups have names such as the alkali metals are the left-most column.
alkali metals = 1st group
alkaline Earth metals = 2nd group
chalcogens = 16th group
halogens = 17th group
noble gases = 18th group
Families tend to be vertical groups but also consider other similarities and thus are not the same as groups. Think of the lanthanide and actinide series etc.
31
What are Chemical families?
Elements that have similar chemical and physical properties, not necessarily part of the same group, but can be.
Alkali metals
Alkaline earth metals
Transition metals
Halogens
Noble gases
For more in depth knowledge:
Science, Tech, Math › Science
Element Families of the Periodic Table

Elements are grouped into families in the periodic table. Digital Art / Getty Images
By
Anne Marie Helmenstine, Ph.D.
Updated on October 27, 2019
Elements may be categorized according to element families. Knowing how to identify families, which elements are included, and their properties helps predict behavior of unknown elements and their chemical reactions.
01
of 10
Element Families

Element families are indicated by numbers located at the top of the periodic table.
Todd Helmenstine
An element family is a set of elements sharing common properties. Elements are classified into families because the three main categories of elements (metals, nonmetals, and semimetals) are very broad. The characteristics of the elements in these families are determined primarily by the number of electrons in the outer energy shell. Element groups, on the other hand, are collections of elements categorized according to similar properties. Because element properties are largely determined by the behavior of valence electrons, families and groups may be the same. However, there are different ways of categorizing elements into families. Many chemists and chemistry textbooks recognize five main families:
5 Element Families
Alkali metals
Alkaline earth metals
Transition metals
Halogens
Noble gases
9 Element Families
Another common method of categorization recognizes nine element families:
Alkali Metals: Group 1 (IA) - 1 valence electron
Alkaline Earth Metals: Group 2 (IIA) - 2 valence electrons
Transition Metals: Groups 3-12 - d and f block metals have 2 valence electrons
Boron Group or Earth Metals: Group 13 (IIIA) - 3 valence electrons
Carbon Group or Tetrels: - Group 14 (IVA) - 4 valence electrons
Nitrogen Group or Pnictogens: - Group 15 (VA) - 5 valence electrons
Oxygen Group or Chalcogens: - Group 16 (VIA) - 6 valence electrons
Halogens: - Group 17 (VIIA) - 7 valence electrons
Noble Gases: - Group 18 (VIIIA) - 8 valence electrons
32
What is the first group of the periodic table called?
Alkali metals
33
What are the characteristics of alkali metals?
- Soft (in comparison, alkaline earth metals are slightly harder than Alkali metals)
- Shiny
- Silver
Metals are insoluble in water or organic solvents, unless they undergo a reaction with them. Typically, this is an oxidation reaction that robs the metal atoms of their itinerant electrons, destroying the metallic bonding.
34
What are alkali metals very reactive with?
Water. For example sodium and water produce an explosion and hydrogen gas is a product.
Also they react commonly with Halogens to make ionic compounds. For example sodium chloride is table salt.
35
What do alkali metal compounds tend to look like?
White solids
36
What are chemical compounds?
A combination of two or more elements combined in a specific ratio
37
What is the second group of the periodic table?
Alkaline Earth metal
38
What are the physical characteristics of alkaline earth metals?
- Shiny
- Silver
- Kind of soft
- Not very soluble in water
39
What is the non-reactive group of elements called?
Noble gases
40
Where are the noble gases located on the periodic table?
The very last column on the right.
41
What are some characteristics of noble gases?
- Non-reactive
- Not dense
- Non-flammable
42
Why are noble gases unable to combust?
They are not reactive since they already have a full outer shell of electrons. Combustion is a chemical reaction so noble gases cannot combust.
43
What group is adjacent (to the left) of the noble gases?
Halogens
44
What are the characteristics of halogens?
- Poisonous
- Reactive with alkali metals
45
What are the three kinds of subatomic particles?
- Electrons
- Protons
- Neutrons
46
What are neutrons?
Neutral particles that add mass
47
What are electrons?
Negatively charged particles with so little mass that they are said to have no mass
48
What are protons?
Positively charged particles
49
Where are the protons and neutrons located?
The nucleus; so the protons and neutrons are called nucleons
50
What are energy levels of an atom?
A region of space near the nucleus that may be empty or contain electrons
51
How do you know the energy of electrons?
- Electrons further away from the nucleus have more energy
- Electrons closest to the nucleus have less energy
When electrons change position they can emit light which helps to see their energy level.
52
Why are electrons closest to the nucleus held tightly?
Because they are closest to protons and the opposite charges attract each other.
53
What is the organization of the levels of electrons?
2, 8, 8, 18, 18, 32, 32
Find this by counting the amount of elements in each row of the periodic table
(There is more to learn here later about the organization of the electrons but this knowledge is sufficient for grade 10; you only need to memorize the first four rows)
54
How do elements bond? Explain what the electrons do.
There are two main types of bonding, with a grey area in between.
Covalent/molecular bonding:
Partly filled energy levels from two different atoms can overlap and electrons can exist in both of them at once. This is called covalent bonding or molecular bonding. The result is a molecule. Two or more non-metals will form a covalent bond.
Ionic bonding:
Also, ionic bonds can occur. This is where one element steals one or more electrons from another element and then the resulting ions carry opposite charges making them stick to each other due to their opposite charges. A common example of an ionic bond is NaCl which is table salt. The sodium gives away an electron to the chlorine so that they can each have an outer shell that resembles that of the closest noble gas. Ionic bonds involve one metal element (duplicates of this metal are allowed).
55
What does the atomic number tell you?
The number of protons an element has
56
What are isotopes?
Atoms of the same element that contain different numbers of neutrons
57
What is heavy hydrogen?
An isotope of hydrogen that contains 1 neutron, since usually hydrogen would just have one proton and one electron, it is heavier when it also has the neutron. Look at the atomic mass number of hydrogen and you will see that it is common to not have the neutron.
58
What does the mass number tell you?
The amount of protons and neutrons (the number of nucleons) in an atom
59
How can the atomic symbol of an element be represented without being in the periodic table
- Mass number (top left)
- Element symbol (right)
- Atomic number (bottom left)
This is the nuclear model of the atom
60
What is the atomic mass (also known as the atomic molar mass)?
The average mass of the isotopes of an element (so notice that the amount of neutrons can change and it is still the same element)
61
What is ionization?
When elements gain or lose electrons
62
What is an ion?
An unbalanced or electrically charged atom (it does this to achieve an outer shell like the nearest noble gas)
63
What does ionization create? What sections of the periodic table participate in this type of compound?
Metals and non-metals form ionic compounds
64
What are cations?
Positively charged atoms that form when atoms lose electrons represented by 1+ or 2+ etc.
Notice that the positive sign goes after the number.
65
What are anions?
Negatively charged atoms that form when atoms gain electrons represented by 1- or 2- etc.
Notice that the negative sign goes after the number.
66
Why do atoms gain and lose electrons?
So they can become stable like noble gasses creating full outer shells of electrons
67
What are valence electrons?
The electrons in the outer energy layer of an atom
68
What does valence mean?
The tendency to gain or lose electrons
69
What is the octet rule?
When atoms bond in such a way that they are able to have 8 electrons in their outer layer
70
Who is responsible for developing the naming system for ionic compounds?
IUPAC the International Union of Pure and Applied Chemistry
71
How do ionic compounds form?
When electrons transfer from one atom to another
72
What physically forms when two kinds of ions group together?
A crystal lattice
73
How do you name ionic compounds?
1) Name the cation
2) Name the anion and change the ending to ide
3) Balance the charges if the cation can take more than one charge to determine which charge it has then put that number in Roman numerals in brackets
74
What are multivalent ions?
Elements with more than 1 stable ion
75
How do you know what the charge is with multivalent ions?
They use Roman numerals in the name
The possible charges are listed on the periodic table
76
What are polyatomic ions?
Several non-metallic atoms joined together
77
What are the most common suffixes for polyatomic ions?
-ate and -ite
78
What is a molecule?
When two or more non-metallic atoms bond together
79
What state can molecular compounds exist in?
Solid, liquid, or gas
80
What are covalent bonds?
When atoms share electrons
81
What is a molecular element? List them along with their states
When atoms form molecules made up of only one atom such as N2 (g) (2 is subscript)
You must memorize these along with their state:
H2 (g)
N2 (g)
O2 (g)
F2 (g)
Cl2 (g)
Br2 (l)
I2 (s)
At2 (s)
P4 (s)
S8 (s)
82
What does diatomic mean?
Only composed of two atoms
E.g. H2 (g) (2 is subscript)
di = 2 atomic = has atoms
83
what are the prefixes for numbers 1-10 as used in covalent bond naming?
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
84
What are the properties of ionic compounds?
- High melting and boiling points
- Retention of crystal shape
- High solubility
- High conductivity
85
What is a precipitate?
A solid with a low solubility that forms a solid in a solution and thus falls out of the solution as it is being created in the chemical reaction
86
What is an electrolyte?
Any solution that can conduct electricity
87
What are the properties of molecular compounds?
- Low melting and boiling points
- Weak bonds in comparison to ionic bonds
- Not conductive
- insoluble in water but soluble in organic solvents
88
What does polar mean?
Each molecule has a positive and negative end (they have two poles)
89
What is an example of a product that is safe until thrown away?
Batteries that contain mercury
90
What are chlorofluorocarbons?
Non-toxic flammable chemicals used mainly in cooling systems. CFCs contain chlorine, fluorine, and carbon in various proportions. CFCs damage the ozone layer.
91
What is the problem with chlorofluorocarbons?
They are catalysts in the upper atmosphere and cause destruction of the Earth's ozone layer
92
What are the two most common recreational substances?
Alcohol and Nicotine
93
Why is alcohol considered to be a drug?
Because of its affects on the body
94
How does alcohol affect the body?
Destruction of liver, kidneys, and brain cells
95
What is physical dependance?
Aka addiction. When body becomes used to a drug and needs it to function
96
What is psychological dependence?
When the use of the drug is linked to certain moods or feelings and when the drug wears off the feeling disappears
97
What is nicotine?
A highly addictive chemical present in all tobacco products
98
What chemicals in cigarettes make them dangerous?
-Large amounts of carbon dioxide
-carbon monoxide
-Tar (A dark, oily, viscous material, consisting mainly of hydrocarbons, produced by the destructive distillation of organic substances such as wood, coal, or peat.)
-Formaldehyde (Formaldehyde is an organic compound with the formula CH₂O and structure H−CHO. The compound is a pungent, colourless gas that polymerises spontaneously into paraformaldehyde.)
-Benzene (C6H6 in a ring of carbons with double and single bonds. Benzene is a chemical that is a colorless or light yellow liquid at room temperature. It has a sweet odor and is highly flammable. Benzene evaporates into the air very quickly. Its vapor is heavier than air and may sink into low-lying areas. Benzene dissolves only slightly in water and will float on top of water.)
99
What body systems are damaged by smoking?
Respiratory and circulatory
100
What is an acid?
A compound that dissolves in water to form a Ph lower than 7
101
What is a base?
A compound that dissolves in water to form a Ph of greater than 7
102
What Ph is saliva?
It is highly basic so that your teeth won't dissolve
103
What type of acid does the stomach make?
Hydrochloric acid strong enough to burn
104
What does the hydrochloric acid in your stomach do?
- Dissolves food
- Turns on an enzyme called pepsin (pepsin facilitates breaking down proteins into amino acids and thus speeds up digestion)
105
What does pepsin do in your stomach?
Speeds up digestion of protein into amino acids
106
What would happen if pepsin was not deactivated before reaching the intestines?
The pepsin would digest the digestive tract
107
What does the pancreas produce?
Sodium Hydrogen Carbonate
The chemical or molecular formula of Sodium Hydrogen Carbonate is NaHCO3. It is a crystalline solid white in colour which has no odour.
Baking soda is the common name of sodium bicarbonate. The chemical formula of baking soda is NaHCO3. Baking Soda is also defined as Sodium Bicarbonate.
Sodium bicarbonate (IUPAC name: sodium hydrogen carbonate), commonly known as baking soda or bicarbonate of soda, is a chemical compound with the formula NaHCO3
108
What does sodium hydrogen carbonate do in the body?
It neutralizes the stomach acid and the pepsin
109
What does the sodium hydrogen carbonate do after neutralizing the stomach acid?
It goes into the bloodstream making it slightly basic
Sodium hydrogen carbonate is also known as baking soda.
110
What is a buffer?
A substance that can keep the pH of a substance nearly constant despite the addition of a small amount of an acid or base
111
What do acidic solutions taste like?
Sour
112
What do basic solutions taste like?
Bitter
113
What do basic solutions feel like?
Slippery
114
What do acidic solutions feel like?
Not slippery that's for sure! Don't touch these!
115
What is a way to detect whether a substance is an acid or base?
Using a piece of metal. Acids try to dissolve metal while bases don't do anything
116
What are the properties of acids?
- Sour
- Not slippery
- Corrodes metal
- Red litmus
- Conductive
- < 7
117
What are the properties of bases?
- Bitter
- Slippery
- No reaction to metals
- Blue litmus
- Conductive
- > 7
118
What are acid-base indicators?
Chemicals that are used to tell if solutions are acidic or basic
119
What is litmus?
A paper that changes color depending on acidity
120
What do the colors of litmus paper represent?
```
Red = Acid
Blue = Base
```
121
What is a universal indicator?
A mixture of several indicators that change color at a specific acidity
122
What is the acidity of stomach acid?
1.5
123
What is the acidity of vinegar?
3
124
Every increase of one on the pH scale means what?
An increase of 10 times the previous
125
How can you identify an acid in a chemical formula containing hydrogen?
- If the H appears on the left
- If COOH appears on the right
126
Why do most acids have aqueous at the end?
Because IUPAC reccomends it
127
What is a popular naming system for acids containing hydrogen and one other element?
If it has one metal they start it with hydro- and end it with -ic
eg. Hydro-chlor-ic acid
128
How can you recognize a basic solution from its chemical formula?
- An OH combined with a metal is usually Basic
- high solubility so likely has aq listed as the state (but keep in mind that acids also have this notation)
129
What is neutralization?
When acids and bases mix together and they lose all their acidic and basic compounds
130
What is the chemical formula and state for ammonia?
NH3 (g)
131
What is the chemical formula and state for glucose?
C6H12O6 (s)
132
What is the chemical formula and state for sucrose?
C12H22O11 (s)
133
What is the chemical formula and state for methane?
CH4 (g)
134
What is the chemical formula and state for propane?
C3H8 (g)
135
What is the chemical formula and state for acetic acid?
This is vitamin C
CH3COOH (aq)
136
What is the chemical formula and state for hydrogen peroxide?
H2O2 (l)
137
What is the chemical formula and state for ozone?
O3 (g)
138
What is the chemical formula and state for methanol?
CH3OH (l)
139
What is the chemical formula and state for ethanol?
C2H5OH (l)
140
What is the chemical formula for hydrochloric acid?
HCl (aq)
141
What is the chemical formula for sulfuric acid?
H2SO4 (aq)
142
What is the chemical formula for nitric acid?
HNO3 (aq)
N= 3 two less hydrogen
P= 4 one less hydrogen
S= 4 two less hydrogen
143
What is the chemical formula for the polyatomic ion acetate?
CH3COO -
144
What is the chemical formula for the polyatomic ion ammonium?
NH4 +
145
What is the chemical formula for the polyatomic ion benzoate?
C6H5COO -
146
What is the chemical formula for the polyatomic ion borate?
BO3 3-
B = 3 three less hydrogen
147
What is the chemical formula for the polyatomic ion carbonate?
CO3 2-
148
What is the chemical formula for the polyatomic ion hydrogen carbonate?
HCO3 -
149
What is the chemical formula for the polyatomic ion perchlorate?
ClO4 -
150
What is the chemical formula for the polyatomic ion chlorate?
ClO3 -
151
What is the chemical formula for the polyatomic ion chlorite?
ClO2 -
152
What is the chemical formula for the polyatomic ion hypochlorite?
ClO -
153
What is the chemical formula for the polyatomic ion chromate?
CrO4 2-
154
What is the chemical formula for the polyatomic ion dichromate?
Cr2O7 2-
155
What is the chemical formula for the polyatomic ion cyanide?
CN -
156
What is the chemical formula for the polyatomic ion hydroxide?
OH -
157
What is the chemical formula for the polyatomic ion iodate?
IO3 -
158
What is the chemical formula for the polyatomic ion nitrate?
NO3-
159
What is the chemical formula for the polyatomic ion nitrite?
NO2 -
160
What is the chemical formula for the polyatomic ion methanoate?
CHOO -
161
What is the chemical formula for the polyatomic ion oxalate?
OOCCOO 2-
162
What is the chemical formula for the polyatomic ion permanganate?
MnO4 -
Mn=3
163
What is the chemical formula for the polyatomic ion phosphate?
PO4 3-
N= 3 two less hydrogen
P= 4 one less hydrogen
S= 4 two less hydrogen
164
What is the chemical formula for the polyatomic ion silicate?
SiO3 2-
165
What is the chemical formula for the polyatomic ion sulfite?
SO3 2-
166
What is the chemical formula for the polyatomic ion sulfate?
SO4 2-
167
What is the chemical formula for the polyatomic ion hydrogen sulfide?
HS -
168
What is the chemical formula for the polyatomic ion hydrogen sulfate?
HSO4 -
N= 3 two less hydrogen
P= 4 one less hydrogen
S= 4 two less hydrogen
169
What is the chemical formula for the polyatomic ion hydrogen sulfite?
HSO3 -
N= 3 two less hydrogen
P= 4 one less hydrogen
S= 4 two less hydrogen
170
What is the chemical formula for the polyatomic ion thiocyanate
SCN -
171
What is the chemical formula for the polyatomic ion thiosulfate?
S2O3 2-
172
All about ionic compounds
173
All about molecular compounds
174
All about acids:
Empirical (observed during experimental procedures) and theoretical evidence (analysis of empirical evidence creates theoretical evidence)
Naming acids
6 strong acids
