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Chemistry Flashcards

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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)

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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

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3
Q

Families

A

Elements in a family have similar physical and chemical properties, and form similar compounds when they combine with other elements.

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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.

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5
Q

What are the 3 basic parts of an atom?

A

Protons, neutrons, and electrons (subatomic particles)

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6
Q

Where do the protons and neutrons live

A

Protons and neutrons live in the nucleus

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7
Q

Where do electrons live

A

Electrons live in shells that orbit the nucleus

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8
Q

what does neutral mean

A

Neutral means an electric charge of 0

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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

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10
Q

what is the max number of electrons that can go into the first shell

A

2

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11
Q

what is the max number of electrons that can go into the other shells

A

8

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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)

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13
Q

what does the atomic mass tell us

A

The atomic mass is the sum of protons and neutrons

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14
Q

how to calculate number of neutrons

A

Number of neutrons = atomic mass (rounded) - atomic number

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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

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16
Q

anion

A

When an electron is added, the atom becomes negatively charged (anion)

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17
Q

cation

A

When an electron is stripped away, the atom becomes positively charged (cation)

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18
Q

how do you write the electron configuration of magnesium?

A

2, 8, 2 = 12

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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

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20
Q

solid

A

Fixed shape & volume, very little space between particles, strong FOA, do not flow easily

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21
Q

liquid

A

Takes shape of the container, little space between particles, weaker FOA, flows easily

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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

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23
Q

plasma + example

A

Superheated matter – so hot that the electrons are ripped away from the atoms forming an ionized gas

ex. lightning

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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

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25
Q

changing between states

A

solid - liquid = melting
liquid - gas = evaporating
solid - gas = sublimation

gas - liquid = condensing
liquid - solid = freezing
gas - solid = deposition

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26
Q

what are physical properties

A

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.

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27
Q

list physical properties (13)

A

State
Colour
Odour
Clarity
Lustre
Brittleness
Malleability
Conductivity
Ductility
Viscosity
Melting or freezing point
Boiling point or boiling range
Density

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28
Q

pure substances

A

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.

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29
Q

mixtures/impure substances part 1

A

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.

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30
Q

mixtures/impure substances part 2

A

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.

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31
Q

the tyndall effect

A

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.

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32
Q

particle theory of matter

A
  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
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33
Q

alkali metals (group 1)

A

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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34
Q

alkaline earth metals (group 2)

A

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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35
Q

halogens (group 17)

A

coloured non-metals that are very reactive

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36
Q

noble gases (group 18)

A

non-metals that are colourless, odourless gases and very unreactive. An unreactive atom does not combine easily with other atoms.

37
Q

what is an ion

A

An ion is an atom or a group of atoms that has a charge.

38
Q

what is an ionic compound

A

transferring of electrons between a metal and a non-metal.

Ionic compounds begin with a metal OR AN AMMONIUM ION (NH4+)

39
Q

what are multivalent metals + transition metals

A

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
Q

how do u distinguish multivalent metals + how many are in a compound?

A

Use roman numerals from I-VII to distinguish between the ion forms

There is only 1 multivalent metal in a compound

41
Q

what is a molecule

A

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
Q

how do u form a molecular compound

A

To form a molecular compound, electrons are shared instead of transferred by two non-metals.

43
Q

rules for molecular compounds

A

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
Q

what are the types of covalent bonds

A

single bonds (1 pair, shares 2e-), double bonds (2 pairs, shares 4e-), triple bonds (3 pairs, shares 6e-)

45
Q

HOFBrINCl

A

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
Q

what are the greek prefixes

A

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
Q

water, ammonia, and methane

A

H20, NH3, CH4

48
Q

diagram of elements vs compounds

A

elements (O O O O O)
Compounds (OOO OOO OOO)

49
Q

diagram of homogenous vs heterogeneous

A

homogenous:
- water + salt = brine
- copper + tin = bronze

heterogenous:
(OOO OOO)

50
Q

what are polyatomic ions

A
  • 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
51
Q

oxyacids

A
  • Polyatomic Ions form oxyacids
  • Hydrogen is used to balance out the charge
  • Ex. HNO₃ (aq) is nitric acid
52
Q

peroxides

A
  • 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
Q

binary acids

A
  • 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
Q

counting atoms

A
  • 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
Q

chemical equations rules

A

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
Q

how do u balance chemical equations?

A

Start with the metals and keep polyatomic ions together, and leave hydrogen and oxygen for the end

57
Q

how do u know a chemical reaction has occured

A
  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
Q

what are not examples that a chemical reaction has occured

A
  1. Changes in state
  2. Changes in size/shape
  3. Change in amount (volume/mass)
59
Q

what are the 5 types of chemical reactions

A

synthesis, decomposition, single replacement/displacement, double replacement/displacement, combustion

60
Q

synthesis

A

A + B → AB

61
Q

decomposition

A

A compound is broken down into simpler compounds

AB → A + B

62
Q

Single Replacement/Displacement

A

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
Q

Double Replacement/Displacement

A

AB + CD → AD + CB

64
Q

combustion

A

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
Q

the fire triangle

A

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
Q

endothermic vs exothermic

A

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
Q

what is IUPAC?

A

Internation Union of Pure and Applied Chemistry - develops rules for naming compounds

68
Q

Catalyst + Indicator:

A
  • 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
Q

The pH Scale:

A
  • 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
Q

Acid Rain:

A

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.

71
Q

The Dangers of Acid Rain on Human:

A

Health issues including respiratory diseases (asthma, bronchitis)
Not strong enough to burn skin

72
Q

dangers of acid rain on environment

A
  • 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
Q

Acids of Acid Rain:

A

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
Q

general and physical properties of acids and bases

A
  • Dissolve in water
  • Conduct electricity in an aqueous solution
  • Can irritate/burn skin
75
Q

general and physical properties of acids

A
  • Taste sour
  • Do not feel slippery
  • Turn blue litmus paper red
  • Releases hydrogen ions in an aqueous solution
  • Are corrosive
76
Q

general and physical properties of bases

A
  • Taste bitter
  • Feel slippery
  • Turn red litmus paper blue
  • Release hydroxide ions in aqueous solution
  • Are not corrosive
77
Q

indicators of acids/bases/neutral

A

Bromythmol blue turns acids yellow, bases blue, and neutrals green

Phenolphthalein turns acids colourless, bases pink, and neutrals colourless

78
Q

Neutralization:

A

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
Q

conservation of mass

A
  • 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
Q

density of water

A

Density is a physical property, and as such, should remain the same regardless of shape or volume

81
Q

test for h2 gas

A

lighted splint will pop in h2 (g)

82
Q

test for o2 gas

A

glowing splin relights in oxygen gas

83
Q

electron configuration of carbon

A

shared

84
Q

electron configuration of helium

A

2, 8

85
Q

lewis dot of helium ion

A

not possible

86
Q

lewis dot of carbon ion

A

not possible

87
Q

overall charge of carbon ion

A

not possible

88
Q

overall charge of helium ion

A

0

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