Chemistry Flashcards
1
Q
What is the exploding bomb? (WHMIS)
A
explosion and reactivity hazard
2
Q
What is the gas cylinder? (WHMIS)
A
gases under pressure hazard
3
Q
What is health hazard? (WHMIS)
A
May cause serious health effects
4
Q
What is flame? (WHMIS)
A
Fire hazard
5
Q
What is corrosion? (WHMIS)
A
Corrosive materials hazard
6
Q
What is the exclamation point? (WHMIS)
A
May cause less serious health effects or damage to the ozone layer
7
Q
What is flame over circle? (WHMIS)
A
Oxidizing hazard
8
Q
What is skull and crossbones? (WHMIS)
A
Small amounts can cause death/toxicity
9
Q
What is ‘‘harmful to the environment’’? (WHMIS)
A
may cause damage to the environment
10
Q
What is biohazardous infectious materials? (WHMIS)
A
organisms/toxins that can cause diseases
11
Q
What does WHMIS stand for?
A
Workplace hazardous materials information system
12
Q
What does HHPS stand for?
A
Hazardous household products symbols
13
Q
What is matter?
A
Anything that takes up space and has a mass; only thing that isn’t matter is energy
14
Q
What are properties?
A
characteristics/traits/attributes
15
Q
What are physical properties?
A
things we can observe with our senses
16
Q
examples of physical properties?
A
- boiling/condensation point
- malleability
- colour
- solubility
- conductivity
- melting/freezing point
- ductility
- crystal formation
- magnetism
17
Q
What is physical change?
A
Changing a substance without changing its composition. (ex. folding paper, chopping wood)
18
Q
What are chemical properties?
A
How it reacts with other substances
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
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)
21
Q
What are pure substances?
A
contain only one type of particle and cannot be physically broken down into another substance
22
Q
What are mixtures?
A
contain two or more pure substances
23
Q
What is homogenous?
A
prefix ‘‘homo’’ means the same. Look the same throughout, cannot be separate components
24
Q
What is heterogenous?
A
prefix ‘‘hetero’’ means different. can see different components
25
What are elements?
made up of one type of atom
26
What are compounds?
Made up of two or more elements chemically combined in specific ratios
27
What are solutions?
A mixture that appears to be made up of only one substance
28
What are mechanical mixtures?
Can easily sort out the different components mechanically
29
What are suspensions?
solid component suspended in liquid component; particles large enough to settle to bottom
30
What are colloids?
Similar to suspension but suspended particles are much smaller and won't settle, often gel-like
31
What did John Dalton find?
'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
32
What did J.J. Thomson find?
'The Plum Pudding Model'
- atoms have one large positive with many small negative charges embedded in it
33
What did Ernest Rutherford find?
'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
34
What did Neils Bohr find?
'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
35
What is the electron cloud model?
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
36
What are subatomic particles?
Protons, electrons, neutrons; particles that make up atoms
37
Where are protons located?
in the nucleus
38
Where are electrons located?
orbiting nucleus
39
Where are neutrons located?
in the nucleus
40
How do you find the number of protons?
the atomic number
41
How do you find the number of electrons?
equal to the number of protons
42
How do you find the number of neutrons?
mass - protons
[mass number - atomic number]
43
Can the number of protons change?
No, the number of protons is the difference of elements (atomic number)
44
Can the number of electrons change?
Yes, elements come together to form ions and gain or lose electrons
45
Can the number of neutrons change?
Yes, an element can exist in different mass; the mass on the periodic table is the most common mass
46
What can we get from the periodic table?
- 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)
47
What are properties of metals?
- shiny, metallic lustre
- good conductors of heat and electricity
- malleable and ductile
- solid at room temp (except mercury)
48
What are properties of non-metals?
- dull
- don't conduct heat well, don't conduct electricity at all
- brittle
- can be any state at room temp.
49
What are properties of metalloids?
- characteristics of both metals and non-metals
- often brittle solids
- conduct electricity, but not as well as metals
50
What are rows/periods?
They go from 1-7 and show the number of energy levels/rings
51
What are columns/groups/families?
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)
52
Properties of group1?
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
53
Properties of group 2?
Alkali Earth Metals
- shiny, silver, not as soft as group 1
- still quite reactive, but not as much as group 1
54
Properties of group 3~16?
Transition Metals
- don't fit rules as easily, left for higher course
55
Properties of group 17?
Halogens
- most are gases except bromine (liquid)
- extremely poisonus
- react easily with alkali metals to form salts
56
Properties of group 18?
Noble Gases
- gases
- inert (unreactive)
57
What are isotopes ?
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
How do you draw Bohr diagrams/
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
How do you draw energy level diagrams?
Basically the Bohr diagram but instead of rings, just draw a line and the number of electrons over it
60
What is the octet rule?
Atoms want to be like their nearest noble gas; have a full outer ring or lose electrons for an empty ring
61
What is an ion?
An atom that lost or gained electrons
62
What are anions?
Negatively charged ions
63
What are cations?
Positively charged ions
64
What do metal atoms become?
They are closer to losing electrons, they become cat ions
65
What do non-metals become?
They are closer to a full shell (gaining electrons), they become anions
66
What are properties of ionic compounds?
- 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
How do you name ionic compounds?
1) write the name of the metal (positive) ion
2) write the name of the non-metal and chagne the ending to -ide
68
How do you write formulas for ionic compounds?
1) write abbreviation of metal ion
2) write abbreviation of non-metal
3) balance charges and write your subscripts (charges must equal 0)
69
What are superscripts?
They tell us the charge of an ion
70
What are subscripts?
They tell us how many of each ion we have
71
What are multivalent elements?
They have multiple possible charges, must use roman numbers in the name
72
What are polyatomic ions?
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
What are ionic compounds?
Compounds made up of a metal and non-metal, ions lose or gain valence electrons to form bonds
74
What are molecular compounds?
Compounds made up of two non-metals, ions share valence electrons to form bonds (covalent bonds)
75
What are properties of molecular compounds?
- 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
How do you name molecular compounds?
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
What is monoatomic?
Elements exist in nature as single atoms
78
What is diatomic?
elements form covalent bonds between themselves and exist as diatomic elements
79
What are common molecular compounds?
Water H2O
Ammonia NH3
Ethanol C2H5OH
Methane CH4
Glucose C6H12O6
Sucrose C12H22O11
80
What are polar molecules?
Has a negative and positive end
81
What types of bonds do water molecules have?
Hydrogen bonds
82
What are 2 unique properties of water that effect Earth?
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
What is solubility?
Measure of how well a substance dissolves in a solvent
84
Why do we mix substances with water when performing chemical reactions?
To speed up the reactions, most ionic compounds dissolve in water, some more than others
85
What is a precipitate?
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
What is aqueous?
(aq) disolves in water; an ion is more attracted to the water molecules
87
How do you use a solubility chart?
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
What is an acid?
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
What is a base?
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
What are properties of an acid?
- 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
What are properties of a base?
- 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
What is the pH scale?
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
What are indicators?
Chemicals that change colour depending on pH (litmus only says if something is an acid, base, or neutral, not the actual pH
94
What are universal indicators?
They turn a range of colours so you can determine the pH
95
What is neutralization?
you mix an acid and base and they cancel each other to make neutral substances (make water and a salt)
96
How do you name acids using the IUPAC system?
International Union of Pure and Applied Chemistry; name it like a regular ionic compound, but put ''aqueous'' in front.
97
How do you name acids using the classical system?
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
How do you know if a neutral substance is ionic or molecular?
If it conducts electricity it is ionic, if it does not conduct electricity, it is molecular.
99
Evidence of chemical change?
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
What is exothermic?
Heat is released, feels hot
101
What is endothermic?
Heat is absorbed, feels cold
102
What is the law of conservation of mass?
- 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
What are the three ways to write chemical equations?
1) sentence form
2) word equation
3) chemical equation
104
what are coefficients?
The big number in front of an entire compound/element; tells us how many of that compound/element there is
105
What are subscripts?
the small number behind an individual element; tells us the ratio of that element within a compound
106
How is every equation formatted?
reactants-> products
107
What is formation/synthesis?
two elements come toegether to form a compound; the reactants are two elements
108
What is decomposition?
a compound breaking down into its 2 elements; only one reactant
109
What is single replacement?
a single element replaces an element in a compound; reactants are one element and one compound (AB + C -> CB + A)
110
What is double replacement?
an element from each of the two compounds switch places; reactants are two compounds (AB + CD -> AD + CB)
111
What is hydrocarbon combustion?
A hydrocarbon burns in the prescence of oxygen to create carbon dioxide and water vapour; always a
hydrocarbon+oxygen->carbon dioxide+water
112
How do you balance a hydrocarbon combustion equation?
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
What are all masses on the periodic table measured in?
grams/mole
114
What is the mole?
Also called 'Avogadro's Number' it is the amount of particles/atoms in 12g of carbon.
1 mole = 6.02*10^23
115
What is molar mass?
The mass on the periodic table; mass of one mole of that element
116
What is n?
number of moles (mol)
117
What is m?
mass (g)
118
What is M?
molar mass (g/mol)
119
What are the three types of thermal energy transfer?
- radiation
- conduction
- convection
120
What is radiation?
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
What is conduction?
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
What is convection?
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
What is specific heat capacity?
Amount of energy required to raise the temperature of 1 gram of substance by 1 degrees celsius
124
What is quantity of thermal energy?
amount of thermal energy released by 1 gram of a substance when its temp. changed by 1 degrees celsius
125
What is Q?
Thermal energy ( J )
126
What is c?
specific heat capacity (J/g degrees celsius)
127
What is Δt?
change in temp (degrees celsius)
128
What does adding energy usually do?
makes a substance hotter
129
When does a phase change occur?
At two specific temperatures, different to each substance
130
What are the phase changes?
1) evaporation
2) condensation
3) freezing
4) melting
5) deposition
6) sublimation
131
What is the heat of fusion?
amount of energy released or absorbed when a substance changes between a solid and liquid
132
What is the heat of vaporization?
Amount of energy released or absorbed when a substance changes between a liquid and gas
