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Chemistry Flashcards

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1
Q

What is the exploding bomb? (WHMIS)

A

explosion and reactivity hazard

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2
Q

What is the gas cylinder? (WHMIS)

A

gases under pressure hazard

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3
Q

What is health hazard? (WHMIS)

A

May cause serious health effects

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4
Q

What is flame? (WHMIS)

A

Fire hazard

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5
Q

What is corrosion? (WHMIS)

A

Corrosive materials hazard

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6
Q

What is the exclamation point? (WHMIS)

A

May cause less serious health effects or damage to the ozone layer

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7
Q

What is flame over circle? (WHMIS)

A

Oxidizing hazard

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8
Q

What is skull and crossbones? (WHMIS)

A

Small amounts can cause death/toxicity

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9
Q

What is ‘‘harmful to the environment’’? (WHMIS)

A

may cause damage to the environment

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10
Q

What is biohazardous infectious materials? (WHMIS)

A

organisms/toxins that can cause diseases

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11
Q

What does WHMIS stand for?

A

Workplace hazardous materials information system

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12
Q

What does HHPS stand for?

A

Hazardous household products symbols

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13
Q

What is matter?

A

Anything that takes up space and has a mass; only thing that isn’t matter is energy

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14
Q

What are properties?

A

characteristics/traits/attributes

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15
Q

What are physical properties?

A

things we can observe with our senses

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16
Q

examples of physical properties?

A
  • boiling/condensation point
  • malleability
  • colour
  • solubility
  • conductivity
  • melting/freezing point
  • ductility
  • crystal formation
  • magnetism
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17
Q

What is physical change?

A

Changing a substance without changing its composition. (ex. folding paper, chopping wood)

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18
Q

What are chemical properties?

A

How it reacts with other substances

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19
Q

Examples of chemical properties?

A
  • ability to burn
  • reaction with oxygen
  • reaction with acids
  • reaction to limtus
  • flashpoint (temp. it ignites at)
  • reaction with water
  • reaction to heat
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20
Q

What is chemical change?

A

Creating a new substance with new properties; happens through a chemical reaction (ex. combining sodium and chlorine to make sodium chloride)

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21
Q

What are pure substances?

A

contain only one type of particle and cannot be physically broken down into another substance

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22
Q

What are mixtures?

A

contain two or more pure substances

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23
Q

What is homogenous?

A

prefix ‘‘homo’’ means the same. Look the same throughout, cannot be separate components

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24
Q

What is heterogenous?

A

prefix ‘‘hetero’’ means different. can see different components

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25
Q

What are elements?

A

made up of one type of atom

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26
Q

What are compounds?

A

Made up of two or more elements chemically combined in specific ratios

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27
Q

What are solutions?

A

A mixture that appears to be made up of only one substance

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28
Q

What are mechanical mixtures?

A

Can easily sort out the different components mechanically

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29
Q

What are suspensions?

A

solid component suspended in liquid component; particles large enough to settle to bottom

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30
Q

What are colloids?

A

Similar to suspension but suspended particles are much smaller and won’t settle, often gel-like

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31
Q

What did John Dalton find?

A

‘The Billiard Ball Model’
- all elements are made up of atoms
- atoms are tiny invisible particles
- all atoms of one element are equal
- atoms combine in ratios to make compounds

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32
Q

What did J.J. Thomson find?

A

‘The Plum Pudding Model’
- atoms have one large positive with many small negative charges embedded in it

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33
Q

What did Ernest Rutherford find?

A

‘The Planetary/Nuclear Model’
- every atom has a positive core that is dense and tiny; the nucleus
- negative charges orbit the nucleus like planets around the sun

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34
Q

What did Neils Bohr find?

A

‘The Bohr Model’
- electrons don’t randomly orbit the nucleus, they are arranged around it in very specific orbits, or energy levels
- positive nucleus, energy levels, and electrons

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35
Q

What is the electron cloud model?

A

what the scientists believe; we do not know exactly where electrons are. Rings suggested by Bohr has the highest probability of an electron being there

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36
Q

What are subatomic particles?

A

Protons, electrons, neutrons; particles that make up atoms

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37
Q

Where are protons located?

A

in the nucleus

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38
Q

Where are electrons located?

A

orbiting nucleus

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39
Q

Where are neutrons located?

A

in the nucleus

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40
Q

How do you find the number of protons?

A

the atomic number

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41
Q

How do you find the number of electrons?

A

equal to the number of protons

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42
Q

How do you find the number of neutrons?

A

mass - protons
[mass number - atomic number]

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43
Q

Can the number of protons change?

A

No, the number of protons is the difference of elements (atomic number)

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44
Q

Can the number of electrons change?

A

Yes, elements come together to form ions and gain or lose electrons

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45
Q

Can the number of neutrons change?

A

Yes, an element can exist in different mass; the mass on the periodic table is the most common mass

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46
Q

What can we get from the periodic table?

A
  • elements’ names and symbols
  • elements’ masses
  • how many electrons/protons/neutrons an element has
  • what state each element is at room temp.
  • whether it is a metal, non-metal, or metalloid (metal is LEFT of staircase, non-metal is RIGHT)
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47
Q

What are properties of metals?

A
  • shiny, metallic lustre
  • good conductors of heat and electricity
  • malleable and ductile
  • solid at room temp (except mercury)
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48
Q

What are properties of non-metals?

A
  • dull
  • don’t conduct heat well, don’t conduct electricity at all
  • brittle
  • can be any state at room temp.
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49
Q

What are properties of metalloids?

A
  • characteristics of both metals and non-metals
  • often brittle solids
  • conduct electricity, but not as well as metals
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50
Q

What are rows/periods?

A

They go from 1-7 and show the number of energy levels/rings

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51
Q

What are columns/groups/families?

A

They go from 1-18 and are based off of how reactive they are. (based on how many valence electrons there are; the closer to a full or empty valence ring, the more reactive)

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52
Q

Properties of group1?

A

Alkali metals
- soft, shiny, silver
- highly reactive with water and halogens
- reactivity increases as you move down
- hydrogen is not a metal but included as it shares similar properties

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53
Q

Properties of group 2?

A

Alkali Earth Metals
- shiny, silver, not as soft as group 1
- still quite reactive, but not as much as group 1

54
Q

Properties of group 3~16?

A

Transition Metals
- don’t fit rules as easily, left for higher course

55
Q

Properties of group 17?

A

Halogens
- most are gases except bromine (liquid)
- extremely poisonus
- react easily with alkali metals to form salts

56
Q

Properties of group 18?

A

Noble Gases
- gases
- inert (unreactive)

57
Q

What are isotopes ?

A

Elements that can have different numbers of neutrons
- mass number of an isotope is the number of protosn and electrons in the atom
- they have identical chemical properties, yet very different nuclear properties

58
Q

How do you draw Bohr diagrams/

A

1) Get total number of electrons from atomic number, get total number of rings from row
2) fill inner ring first then fill outside rings clockwise

59
Q

How do you draw energy level diagrams?

A

Basically the Bohr diagram but instead of rings, just draw a line and the number of electrons over it

60
Q

What is the octet rule?

A

Atoms want to be like their nearest noble gas; have a full outer ring or lose electrons for an empty ring

61
Q

What is an ion?

A

An atom that lost or gained electrons

62
Q

What are anions?

A

Negatively charged ions

63
Q

What are cations?

A

Positively charged ions

64
Q

What do metal atoms become?

A

They are closer to losing electrons, they become cat ions

65
Q

What do non-metals become?

A

They are closer to a full shell (gaining electrons), they become anions

66
Q

What are properties of ionic compounds?

A
  • high melting/boiling points (strong bonds)
  • solid at room temp.
  • dissolve in water (positive ions attracted to negative side of water, negative ions to positive side)
  • when dissolved in water, will conduct electricity (charges free to move can carry electric charges)
67
Q

How do you name ionic compounds?

A

1) write the name of the metal (positive) ion
2) write the name of the non-metal and chagne the ending to -ide

68
Q

How do you write formulas for ionic compounds?

A

1) write abbreviation of metal ion
2) write abbreviation of non-metal
3) balance charges and write your subscripts (charges must equal 0)

69
Q

What are superscripts?

A

They tell us the charge of an ion

70
Q

What are subscripts?

A

They tell us how many of each ion we have

71
Q

What are multivalent elements?

A

They have multiple possible charges, must use roman numbers in the name

72
Q

What are polyatomic ions?

A

A group of atoms combined together that exist as a single unit and have a charge (an -ate or -ite ending, except hydroxide)

  • you do not change the ending to -ide when naming and add brackets when adding subscripts
73
Q

What are ionic compounds?

A

Compounds made up of a metal and non-metal, ions lose or gain valence electrons to form bonds

74
Q

What are molecular compounds?

A

Compounds made up of two non-metals, ions share valence electrons to form bonds (covalent bonds)

75
Q

What are properties of molecular compounds?

A
  • have low boiling.melting points (bonds are weak)
  • can be any state at room temp.
  • will crumble easily when broken
  • won’t dissolve in water (no charges for attraction)
  • won’t conduct electricity when dissolved in water (no charges, nothing to conduct electricity)
76
Q

How do you name molecular compounds?

A

1) write the name of the first element
2) write the name of the second element and change the ending to -ide
3) add prefixes indicating number of atoms (don’t use mono on first element though)
4) do not reduce, no need to balance either

77
Q

What is monoatomic?

A

Elements exist in nature as single atoms

78
Q

What is diatomic?

A

elements form covalent bonds between themselves and exist as diatomic elements

79
Q

What are common molecular compounds?

A

Water H2O
Ammonia NH3
Ethanol C2H5OH
Methane CH4
Glucose C6H12O6
Sucrose C12H22O11

80
Q

What are polar molecules?

A

Has a negative and positive end

81
Q

What types of bonds do water molecules have?

A

Hydrogen bonds

82
Q

What are 2 unique properties of water that effect Earth?

A

1) large specific heat capacity (4.19J/g C)
- this is how mmuch energy it takes to raise one gram of a substance by 1C. Having a high specific heat capacity means water can store lots of heat, so oceans have a big effect on weather

2) density of solid state is less than the density of liquid state
- this is why ice floats in water, water is one of the only substances that this is the case for

83
Q

What is solubility?

A

Measure of how well a substance dissolves in a solvent

84
Q

Why do we mix substances with water when performing chemical reactions?

A

To speed up the reactions, most ionic compounds dissolve in water, some more than others

85
Q

What is a precipitate?

A

Labelled as a solid(s), an ion is more attracted to the other ion of its compound than to a water molecule and doesn’t dissolve very much

86
Q

What is aqueous?

A

(aq) disolves in water; an ion is more attracted to the water molecules

87
Q

How do you use a solubility chart?

A

1) locate the second ion at the top of the table
2) look at the columns below and locate the first ion in very soluble (aq) or slightly soluble (s)

  • if you can’t find the ion, it is included in “most”
  • for multivalent ions you must find the specific charge, otherwise it will be in ‘‘most’’
88
Q

What is an acid?

A

A compound that contains hydrogen acting as a metal and dissolves in water to make a solution with a pH less than 7 (state is aqueous and has H at the front of the formula or COOH at the end)

89
Q

What is a base?

A

a compound that dissolves in water to make a solution with a pH more than 7 (state is aqueous and has hydroxide at the end of the formula- not including COOH)

90
Q

What are properties of an acid?

A
  • turn limus paper red
  • taste sour
  • react with metals to form hydrogen gas
  • always dissociate (seperate into ions) when they dissolve
  • solutions conduct electricity
91
Q

What are properties of a base?

A
  • turn litmus paper blue
  • taste bitter
  • feel slippery
  • don’t react with metals
  • always dissociate (separate into ions) when they dissolve
  • solutions conduct electricity
92
Q

What is the pH scale?

A

It is used to measure how acidic/basic a substance is
(the scale is logarithmic, meaning each charge in pH is actually a 10* charge, so a pH of 2 is 10* more than a pH of 3)

93
Q

What are indicators?

A

Chemicals that change colour depending on pH (litmus only says if something is an acid, base, or neutral, not the actual pH

94
Q

What are universal indicators?

A

They turn a range of colours so you can determine the pH

95
Q

What is neutralization?

A

you mix an acid and base and they cancel each other to make neutral substances (make water and a salt)

96
Q

How do you name acids using the IUPAC system?

A

International Union of Pure and Applied Chemistry; name it like a regular ionic compound, but put ‘‘aqueous’’ in front.

97
Q

How do you name acids using the classical system?

A

Name acids based on what ending it has and ignore the hydrogen.

-ite ending? Change it to -ous

-ate ending? Change it to -ic

-ide ending? Change it to -ic and put hydro- in front

98
Q

How do you know if a neutral substance is ionic or molecular?

A

If it conducts electricity it is ionic, if it does not conduct electricity, it is molecular.

99
Q

Evidence of chemical change?

A

1) formation of a gas- if one of the products is a gas, bubbles will appear
2) formation of a precipitate- one of the products isn’t soluble in water
3) change in colour- a new substance with a new colour is formed
4) change in odour- a new substance with a new odour is formed
5) change in energy- heat or light is absorbed/released

100
Q

What is exothermic?

A

Heat is released, feels hot

101
Q

What is endothermic?

A

Heat is absorbed, feels cold

102
Q

What is the law of conservation of mass?

A
  • total number of atoms/ions in the reactants is equal to the total number of atoms/ions in the products
  • bonds of the reactants are broken and new bonds are formed
  • no atoms/ions coming/leaving, just rearranged
103
Q

What are the three ways to write chemical equations?

A

1) sentence form
2) word equation
3) chemical equation

104
Q

what are coefficients?

A

The big number in front of an entire compound/element; tells us how many of that compound/element there is

105
Q

What are subscripts?

A

the small number behind an individual element; tells us the ratio of that element within a compound

106
Q

How is every equation formatted?

A

reactants-> products

107
Q

What is formation/synthesis?

A

two elements come toegether to form a compound; the reactants are two elements

108
Q

What is decomposition?

A

a compound breaking down into its 2 elements; only one reactant

109
Q

What is single replacement?

A

a single element replaces an element in a compound; reactants are one element and one compound (AB + C -> CB + A)

110
Q

What is double replacement?

A

an element from each of the two compounds switch places; reactants are two compounds (AB + CD -> AD + CB)

111
Q

What is hydrocarbon combustion?

A

A hydrocarbon burns in the prescence of oxygen to create carbon dioxide and water vapour; always a
hydrocarbon+oxygen->carbon dioxide+water

112
Q

How do you balance a hydrocarbon combustion equation?

A

1) balance carbon on either side
2) balance hydrogen on either side
3) add up the 2 sets of oxygen on the product side and balance, may need to double all coefficients

113
Q

What are all masses on the periodic table measured in?

A

grams/mole

114
Q

What is the mole?

A

Also called ‘Avogadro’s Number’ it is the amount of particles/atoms in 12g of carbon.

1 mole = 6.02*10^23

115
Q

What is molar mass?

A

The mass on the periodic table; mass of one mole of that element

116
Q

What is n?

A

number of moles (mol)

117
Q

What is m?

A

mass (g)

118
Q

What is M?

A

molar mass (g/mol)

119
Q

What are the three types of thermal energy transfer?

A
  • radiation
  • conduction
  • convection
120
Q

What is radiation?

A

Occurs in gases or a vacuum
- emission of energy as particles or waves
- waves absorved by other objects, particles of that object warm up/ get more energy

121
Q

What is conduction?

A

Occurs in solids
- particles near heat source gians energy and starts vibrating more
- the energy transfers to nearby particles and all particles eventually gain energy

122
Q

What is convection?

A

occurs in fluids (liquids/gases)
- particle near heat source gains energy, moves more
- more space between particles in fluids, energized particles move away from heat source
- colder (higher density) particles move down to new space, now near heat source and gains energy

123
Q

What is specific heat capacity?

A

Amount of energy required to raise the temperature of 1 gram of substance by 1 degrees celsius

124
Q

What is quantity of thermal energy?

A

amount of thermal energy released by 1 gram of a substance when its temp. changed by 1 degrees celsius

125
Q

What is Q?

A

Thermal energy ( J )

126
Q

What is c?

A

specific heat capacity (J/g degrees celsius)

127
Q

What is Δt?

A

change in temp (degrees celsius)

128
Q

What does adding energy usually do?

A

makes a substance hotter

129
Q

When does a phase change occur?

A

At two specific temperatures, different to each substance

130
Q

What are the phase changes?

A

1) evaporation
2) condensation
3) freezing
4) melting
5) deposition
6) sublimation

131
Q

What is the heat of fusion?

A

amount of energy released or absorbed when a substance changes between a solid and liquid

132
Q

What is the heat of vaporization?

A

Amount of energy released or absorbed when a substance changes between a liquid and gas

Science 10-1 (3 decks)

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