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Chem 10 Flashcards

1
Q

WHMIS

A

Workplace Hazardous Materials Information System

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2
Q

SDS (MSDS)

A

Safety Data Sheets (Materials Safety Data Sheets)

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3
Q

Physical Properties

A

describe the appearance and physical composition of a substance

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4
Q

Chemical Properties

A

Describe the reactivity of one substance with another

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5
Q

Types of physical properties

A

-Boiling/melting point
-malleability
-ductility
-colour
-state
-solubility
-crystal formation
-conductivity
-magnetism

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6
Q

Types of chemical properties

A

-Ability to burn
-flash point
-behaviour in air
-reaction with water
-reaction with acid
-reaction to red and blue litmus

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7
Q

Matter

A

Has mass and takes up space

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8
Q

Mixture

A

Physical combination of 2 or more substances, each of which keeps it’s own chemical properties

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9
Q

Homogenous

A

Same appearance throughout- single phase(solid, liquid, gas)- suspension, colloid

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10
Q

Heterogeneous / mechanical mixture

A

Components can be distinguished, not uniform in appearance, possibly more than one phase (solid, liquid, gas)

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11
Q

Solution

A

Composed of a solute and solvent

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12
Q

Colloid

A

Particles do not settle out through time. Cannot see particles with eye. Very thick, sticky.

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13
Q

Suspension

A

Particles in liquid settle out due to gravity. Can see particles with eye

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14
Q

Element

A

Cannot be further decomposed. Represented on the periodic table table by an atomic symbol.

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15
Q

Compound

A

Chemical combination of 2 or more elements. Can be decomposed by a chemical reaction.

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16
Q

Salting

A

Placing meat in salt to preserve it and draw out water and bacteria.

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17
Q

Smoking

A

Creates an antioxidant to preserve the food.

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18
Q

Heating

A

Sterilizes food to make it safe to eat.

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19
Q

Canning

A

Preserves food without oxygen, kills off microbes

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20
Q

Fermentation

A

Biochemical preservation to preserve and create lactic acid to prevent growth of bacteria

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21
Q

Freezing

A

Prevents the growth of bad bacteria, meaning the food will keep for a very long time

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22
Q

Aristotle

A

Believed all matter was made up of air, earth, fire, or water

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23
Q

Democritus

A

Believed all matter was made up of “atomos” (atomos means indivisible)

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24
Q

John Dalton

A

All matter is made up of atoms, atoms of the same element are identical, atoms of different element have different properties, elements can combine into a specific ratio. Billiard Ball Model.

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25
J.J. Thomson
"Plum pudding model" , atom was a sphere of positive charge embedded with negative particles.
26
Nagoaka
Electron found outside the sphere like saturn's rings.
27
Ernest Rutherford
Atom has tiny positively charged nucleus
28
Neils Bohr
Electron travel around the nucleus in discrete models
29
30
Metals
Silver grey and/ or shiny Solid at room temp (except mercury, which is a liquid) React strongly with other substances
31
Non-metals
includes 17 elements(11gases, 5 solids and 1 liquid, bromine, at room temp) vary in colour
32
metalloids
in between metals and non metals
33
Alkali metals
group 1 soft, shiny, silver very reactive with halogens compounds tend to be white solids that are soluble in water
34
Alkaline earth metals
group 2 shiny and silver compounds tend to be white solids that are white but less soluble than alkali metal compounds
35
Noble gases
group 18 non-metals unreactive
36
halogens
group 17 non-metals poisonous and react readily with alkali metals to form salts
37
metal reactivity
more reactive as you move down and left
38
Non- metal reactivity
more reactive as you move up and right
39
3 subatomic particles that make up each atom?
electrons(negatively charged)e- Protons(positively charged)p+ neutrons(neutral, no charge)n
40
what percent of the weight of an atom do protons and neutrons make up?
99.9% in the mass of the atom
41
How many electrons can each energy level in an atom hold?
The lowest can only hold 2 and the others can hold 8 each
42
mass number
indicates the number of protons an atom has
43
Atomic Number
integer equal to the total number of protons and neutrons (p+ + n)
44
Atomic molar mass
found on the periodic table, average mass of the element isotopes
45
Isotopes
atoms of the same element can have different numbers of neutrons, there are different possible versions of these and they are called isotopes
46
common hydrogen isotope
hydrogen isotope with no neutrons
47
deuterium
hydrogen isotope with one neutron
48
tritium
hydrogen isotope with two neutrons
49
Ionization
when an atom loses or gains an electron to have the same number of electrons as the nearest noble gas and to be more stable.
50
Cations
positively charged ions (don't change anything when naming)
51
anions
negatively charged ions (change ending of second element to "ide"
52
if an atom loses an electron...
...it becomes positive
53
if an atom gains an electron...
...it becomes negative
54
valence level
outermost energy level
55
valence electrons
electrons in outermost energy level
56
octet rule
Atoms bond in such a way to have 8 electrons in their energy levels (hydrogen, helium and lithium are exceptions)
57
covalent bond
chemical bond that involves sharing a pair of electrons between atoms in a molecule
58
molecular compound
composed of only non-metals
59
chemical reaction
a process that occurs when a substance or substances react to form a different substance or substances
60
Biochemical reactions
- cellular respiration (exothermic reaction) - photosynthesis (endothermic reaction)
61
Balanced formula equation
The number of atoms on the reactants side must equal the number of atoms on the product side, use coefficients to balance, subscripts DON'T change
62
Skeleton formula equation
shows which substances are involved but does not show proportions
63
Word equation
determine the reactants and products, set up with + and ---> ex: magnesium+hydrochloric acid ---> magnesium chloride + hydrogen gas
64
Formation (synthesis)
single elements or compounds combine to form larger, more complex compounds
65
Decomposition
products are simpler than reactants
66
Hydrocarbon combustion
products are always carbon dioxide and water
67
Single replacement
cations can only switch with cations, anions can only switch with anions
68
Double replacement
exchange of similarly charged ions
69
Mole
a quantity that chemists use to measure elements and compounds, symbol: mol
70
Avogadro's number
the number of atoms or molecules in 1 mol approximately 6.02 x 10^23, symbol: NA
71
Molar mass
the mass of one mole of a substance the atomic molar mass (found on the periodic table) of an element is the average mass of one mole of atoms of that element, Ex: molar mass of carbon is 12.01 g/mol
72
How do you find the molar mass of compounds?
1. list the elements separately 2. find the molar mass of each of the elements 3. multiply the molar mass by how many atoms are presents 4. add the individual molar masses together
73
Molar equation
the number of moles of a substance is related to it's molar mass by the following equation: m= n x M m= mass (grams) , n= quantity of matter (moles) , M= molar mass (g/mol)
74
How to find "n" in the molar equation formula
n= m/M
75
How to find "M" in molar equation formula
M= m/n
76
Molar ratio
the coefficients in a balanced chemical equation indicate the number of moles required for the reaction, Ex: Cl2 (1mol) + H2 (1mol) --->2 HCl (2mol)

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