Chemistry Flashcards
(88 cards)
1
Q
Columns
A
The vertical lines in a periodic table, called a group or a family
All elements in a family have the same # of valence electrons (electrons in the outermost shell)
2
Q
Rows
A
The horizontal lines in a periodic table, called a period.
All elements in a period have the same # of electron shells
3
Q
Families
A
Elements in a family have similar physical and chemical properties, and form similar compounds when they combine with other elements.
4
Q
what is an atom
A
All matter is made up of tiny particles called atoms. An atom is the smallest part of an element.
5
Q
What are the 3 basic parts of an atom?
A
Protons, neutrons, and electrons (subatomic particles)
6
Q
Where do the protons and neutrons live
A
Protons and neutrons live in the nucleus
7
Q
Where do electrons live
A
Electrons live in shells that orbit the nucleus
8
Q
what does neutral mean
A
Neutral means an electric charge of 0
9
Q
what is the point of the neutrons
A
Neutrons purpose is to hold the nucleus together by stopping protons from repelling each other and thus breaking apart the nucleus
10
Q
what is the max number of electrons that can go into the first shell
A
2
11
Q
what is the max number of electrons that can go into the other shells
A
8
12
Q
what does the atomic number tell us
A
The atomic number is the # of protons in the nucleus
(The # of protons is the same as the # of electrons, when the atom has no overall charge)
13
Q
what does the atomic mass tell us
A
The atomic mass is the sum of protons and neutrons
14
Q
how to calculate number of neutrons
A
Number of neutrons = atomic mass (rounded) - atomic number
15
Q
why is electron configuration important?
A
Electron configuration (x, y, … = x+y+…) is important because it affects the properties of the element and how it behaves in the world
16
Q
anion
A
When an electron is added, the atom becomes negatively charged (anion)
17
Q
cation
A
When an electron is stripped away, the atom becomes positively charged (cation)
18
Q
how do you write the electron configuration of magnesium?
A
2, 8, 2 = 12
19
Q
what are the 5 states of matter and what do they have?
A
solids, liquids, gases, plasmas, and Bose-Einstein condensates (BEC).
different physical properties
20
Q
solid
A
Fixed shape & volume, very little space between particles, strong FOA, do not flow easily
21
Q
liquid
A
Takes shape of the container, little space between particles, weaker FOA, flows easily
22
Q
gas
A
Takes the shape of the volume of the container, expands, lots of free space between particles, very weak FOA, flows easily
23
Q
plasma + example
A
Superheated matter – so hot that the electrons are ripped away from the atoms forming an ionized gas
ex. lightning
24
Q
bec + example
A
a state of matter in which separate atoms or subatomic particles, cooled to near absolute zero (0 K, 273.15 °C), coalesce into a single quantum mechanical entity
ex. superfluids
25
changing between states
solid - liquid = melting
liquid - gas = evaporating
solid - gas = sublimation
gas - liquid = condensing
liquid - solid = freezing
gas - solid = deposition
26
what are physical properties
Characteristics of a substance that observed or measured without changing the composition of matter. They are used to observe and describe matter. They are an important part of the SDS.
27
list physical properties (13)
State
Colour
Odour
Clarity
Lustre
Brittleness
Malleability
Conductivity
Ductility
Viscosity
Melting or freezing point
Boiling point or boiling range
Density
28
pure substances
A pure substance is made up of only one type of matter and has a unique set of properties.
Elements are substances that cannot be broken down into anything simpler and are made up of only one type of atom, such as sodium.
Compounds contain 2+ elements that are chemically bonded together, like H2O.
29
mixtures/impure substances part 1
Mixtures are a combination of pure substances.
Homogeneous mixtures consist of 2+ pure substances that are uniform throughout, the different parts of it not visible. Ex. Sugar dissolved in water (solution) or a mixture of metals (alloy)
Heterogeneous mixtures consist of 2+ pure substances that are not chemically bonded and therefore are not uniform.
30
mixtures/impure substances part 2
Colloids (1-1000nm) are a heterogenous mixture in which very small particles of one substance are uniformly distributed and remain suspended throughout another substance, like milk because particles of fat are suspended in milk. They cannot be separated by filtration.
Suspensions (>1000nm) are heterogeneous mixtures of a finely distributed (but not uniformly) solid in a liquid, like chalk in water. The particles can be separated by filtration and settle in the liquid.
31
the tyndall effect
The Tyndall Effect is the scattering of a light beam when passed through a colloidal or suspension mixture. In a solution, the particles are so small (0.01-1nm) that the light does not get scattered and simply passes through.
32
particle theory of matter
1. all matter is made up of very tiny particles
2. all particles in the same type of matter are identical
3. there are spaces in between particles
4. the particles attract each other
5. particles are always moving
33
alkali metals (group 1)
soft, silver-grey metals that react easily with water and with oxygen in the air. Note that hydrogen is not an alkali metal.
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alkaline earth metals (group 2)
silver-grey metals that are harder and less reactive than group 1 metals. A reactive atom combines easily with other atoms.
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halogens (group 17)
coloured non-metals that are very reactive
36
noble gases (group 18)
non-metals that are colourless, odourless gases and very unreactive. An unreactive atom does not combine easily with other atoms.
37
what is an ion
An ion is an atom or a group of atoms that has a charge.
38
what is an ionic compound
transferring of electrons between a metal and a non-metal.
Ionic compounds begin with a metal OR AN AMMONIUM ION (NH4+)
39
what are multivalent metals + transition metals
Some metals are multivalent, meaning they have more than one ion form (more than one charge)
Transition metals are from Group 3 - 12, these are NOT the same as multivalent metals
40
how do u distinguish multivalent metals + how many are in a compound?
Use roman numerals from I-VII to distinguish between the ion forms
There is only 1 multivalent metal in a compound
41
what is a molecule
A molecule is a combination of 2 or more atoms held together by covalent bonds.A covalent bond is a connection, usually between non-metals, in which the two atoms share a pair of electrons
42
how do u form a molecular compound
To form a molecular compound, electrons are shared instead of transferred by two non-metals.
43
rules for molecular compounds
two non-metals
- since they are negatively charged, they will repel, so molecular compounds do not have ions
- The number of electrons that are needed to have a STABLE OCTET OF VALENCE ELECTRONS is found in the same way as with ionic compounds, but this number is now called the combining capacity of the atom
- Binding capacity = the number of electrons to have a full valence shell
44
what are the types of covalent bonds
single bonds (1 pair, shares 2e-), double bonds (2 pairs, shares 4e-), triple bonds (3 pairs, shares 6e-)
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HOFBrINCl
HOFBrINCl are seven elements that are diatomic molecules. A diatomic molecule is a pair of atoms that are joined by covalent bonds because they are more stable than the individual atom.
They have a subscript of 2
46
what are the greek prefixes
The Greek Prefixes are mono, di, tri, tetra, penta, hexa, hepta, octa, nona, and deca
** mono is not needed for the FIRST element, however it is needed for the second **
47
water, ammonia, and methane
H20, NH3, CH4
48
diagram of elements vs compounds
elements (O O O O O)
Compounds (OOO OOO OOO)
49
diagram of homogenous vs heterogeneous
homogenous:
- water + salt = brine
- copper + tin = bronze
heterogenous:
(OOO OOO)
50
what are polyatomic ions
- Ions that are charged/have an overall charge and have more than 1 element/atom
- They are groups of atoms acting as a single atom
- When making a compound,the charges must
balance
- In any compound, the overall charge is 0
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oxyacids
- Polyatomic Ions form oxyacids
- Hydrogen is used to balance out the charge
- Ex. HNO₃ (aq) is nitric acid
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peroxides
- Consist of more than 1 atom, but the atoms (which is oxygen) are the same
- O₂2-
- Ex H₂O is water, but H₂O₂ is hydrogen peroxide
- Ex. BaO is barium oxide, but BaO₂ is barium peroxide
53
binary acids
- Made up of 2 elements only
- The first is always hydrogen
Ex. HCl (aq) is hydrochloric acid
Ex. H₂S (aq) is hydrosulfuric acid
** (aq) denotes that the substance is dissolved in water**
54
counting atoms
- Subscripts multiply everything in the bracket before it
- Ex. (OH)₂ is O₂ and H₂
- Coefficients multiply everything after it
- Ex. 2 CaCO₂ is Ca₂ and C₂ and O₄
55
chemical equations rules
The # of atoms on the left hand side (reactants) is equal to the number of atoms on the right hand side (products)
They are separated by an arrow and a + is used to list the chemicals
Use state symbols to indicate solid (s), liquid (l), gas (g), or aqueous solution (aq)
These equations can ONLY balance with a coefficient in front
56
how do u balance chemical equations?
Start with the metals and keep polyatomic ions together, and leave hydrogen and oxygen for the end
57
how do u know a chemical reaction has occured
1. Bubbles appear (this means a new gas formed without heating)
a. New smell
2. A colour change occurs
3. A precipitate (new solid) forms without cooling
4. Light/heat is absorbed or given off (change in temperature)
5. Irreversible by physical means
58
what are not examples that a chemical reaction has occured
1. Changes in state
2. Changes in size/shape
3. Change in amount (volume/mass)
59
what are the 5 types of chemical reactions
synthesis, decomposition, single replacement/displacement, double replacement/displacement, combustion
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synthesis
A + B → AB
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decomposition
A compound is broken down into simpler compounds
AB → A + B
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Single Replacement/Displacement
AB + C → AC + B
- This is completed using the activity series
- more reactive replaces less reactive
- Fluorine is the most reactive non-metal
- From Mg to Pb (lead), these elements will only replace hydrogen if its in an acid (aq)
63
Double Replacement/Displacement
AB + CD → AD + CB
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combustion
Combines with oxygen to create carbon dioxide and water
CₓHᵧ(Oᵥ) + O₂ → CO₂ + H₂O
- Complete combustion (hydrocarbon + oxygen gas → carbon dioxide gas + water gas)
- Incomplete combustion (hydrocarbon + insufficient oxygen gas → carbon monoxide + water gas)
65
the fire triangle
oxygen (left side) to fuel (bottom side) to heat (right side)
3 things needed to create fire
Heat is a reactant and a product
66
endothermic vs exothermic
Exothermic:
Heat moves from something to surroundings
- Combustion is an exothermic reaction
because it gives off heat
Endothermic:
Heat moves from surroundings to something
- Reactions that result in colder temperatures
because they use more energy than they
release
67
what is IUPAC?
Internation Union of Pure and Applied Chemistry - develops rules for naming compounds
68
Catalyst + Indicator:
- A catalyst is a substance that speeds up a chemical reaction but does not get used up
- An indicator proves the presence of a base/acid
69
The pH Scale:
- Acids have a pH of less than 7
- All acids contain a hydrogen ion
- Distilled water has a pH of 7, it is neutral
- Bases/alkaline have a pH of greater than 7
- All bases contain a hydroxide ion
The pH of a substance can be determined only when it is in aqueous solution (i.e., dissolved in water).
70
Acid Rain:
Acid rain results when sulphur dioxide and nitrogen oxides are emitted into the atmosphere by
- Burning of fossil fuels (⅔ of sulphur dioxide and ¼ of nitrogen oxides come from electric power generators)
- Vehicles and manufacturing
- A small porting comes from natural sources like volcanoes
They are then transformed into acid particles that are transported long distances by wind and air currents. They then fall to the Earth.
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The Dangers of Acid Rain on Human:
Health issues including respiratory diseases (asthma, bronchitis)
Not strong enough to burn skin
72
dangers of acid rain on environment
- Acid rain leaches aluminum from the soil and then flows into water bodies, effectively releasing aluminum from the ecosystem
- Many species, especially the young, are sensitive to low pH levels and cannot survive
- Even if an animal can tolerate acid rain, the animals that eat it might not
- Acid rain also removes minerals and nutrients from the soil that trees need to grow, leaving them to die
- Frogs can survive down to a pH of 4, and are known as an indicator species. No frogs means the environment is very acidic.
73
Acids of Acid Rain:
The reactions are all synthesis reactions
- Sulfur dioxide + oxygen -> sulfur trioxide
- Sulfur trioxide + water -> sulfuric acid
- Nitrogen oxide + water -> nitric/nitrous acid
- Carbon dioxide + water -> carbonic acid
74
general and physical properties of acids and bases
- Dissolve in water
- Conduct electricity in an aqueous solution
- Can irritate/burn skin
75
general and physical properties of acids
- Taste sour
- Do not feel slippery
- Turn blue litmus paper red
- Releases hydrogen ions in an aqueous solution
- Are corrosive
76
general and physical properties of bases
- Taste bitter
- Feel slippery
- Turn red litmus paper blue
- Release hydroxide ions in aqueous solution
- Are not corrosive
77
indicators of acids/bases/neutral
Bromythmol blue turns acids yellow, bases blue, and neutrals green
Phenolphthalein turns acids colourless, bases pink, and neutrals colourless
78
Neutralization:
An acid + a base → H2O (l) + an ionic salt
Eg. HCl (aq) + NaOH (aq) → HOH (l) + NaCl (aq)
This is a form of double displacement reaction.
79
conservation of mass
- Discovery was made by French chemist Antoine
Lavoisier with his wife Marie-Anne Paulze.
- The total mass of reactants and the total mass of
products in a given reaction are always the same
- The mass is neither created nor destroyed, it is
conserved
- The TOTAL mass does not change during a
chemical reaction
- Gas has mass!! So it can be released and
therefore “lower” the mass of the products
80
density of water
Density is a physical property, and as such, should remain the same regardless of shape or volume
81
test for h2 gas
lighted splint will pop in h2 (g)
82
test for o2 gas
glowing splin relights in oxygen gas
83
electron configuration of carbon
shared
84
electron configuration of helium
2, 8
85
lewis dot of helium ion
not possible
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lewis dot of carbon ion
not possible
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overall charge of carbon ion
not possible
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overall charge of helium ion
0
