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Science > Chem 10 > Flashcards

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
Q

J.J. Thomson

A

“Plum pudding model” , atom was a sphere of positive charge embedded with negative particles.

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26
Q

Nagoaka

A

Electron found outside the sphere like saturn’s rings.

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27
Q

Ernest Rutherford

A

Atom has tiny positively charged nucleus

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28
Q

Neils Bohr

A

Electron travel around the nucleus in discrete models

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29
Q
A
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30
Q

Metals

A

Silver grey and/ or shiny
Solid at room temp (except mercury, which is a liquid)
React strongly with other substances

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31
Q

Non-metals

A

includes 17 elements(11gases, 5 solids and 1 liquid, bromine, at room temp)
vary in colour

32
Q

metalloids

A

in between metals and non metals

33
Q

Alkali metals

A

group 1
soft, shiny, silver
very reactive with halogens
compounds tend to be white solids that are soluble in water

34
Q

Alkaline earth metals

A

group 2
shiny and silver
compounds tend to be white solids that are white but less soluble than alkali metal compounds

35
Q

Noble gases

A

group 18
non-metals
unreactive

36
Q

halogens

A

group 17 non-metals
poisonous and react readily with alkali metals to form salts

37
Q

metal reactivity

A

more reactive as you move down and left

38
Q

Non- metal reactivity

A

more reactive as you move up and right

39
Q

3 subatomic particles that make up each atom?

A

electrons(negatively charged)e-
Protons(positively charged)p+
neutrons(neutral, no charge)n

40
Q

what percent of the weight of an atom do protons and neutrons make up?

A

99.9% in the mass of the atom

41
Q

How many electrons can each energy level in an atom hold?

A

The lowest can only hold 2 and the others can hold 8 each

42
Q

mass number

A

indicates the number of protons an atom has

43
Q

Atomic Number

A

integer equal to the total number of protons and neutrons (p+ + n)

44
Q

Atomic molar mass

A

found on the periodic table, average mass of the element isotopes

45
Q

Isotopes

A

atoms of the same element can have different numbers of neutrons, there are different possible versions of these and they are called isotopes

46
Q

common hydrogen isotope

A

hydrogen isotope with no neutrons

47
Q

deuterium

A

hydrogen isotope with one neutron

48
Q

tritium

A

hydrogen isotope with two neutrons

49
Q

Ionization

A

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
Q

Cations

A

positively charged ions (don’t change anything when naming)

51
Q

anions

A

negatively charged ions (change ending of second element to “ide”

52
Q

if an atom loses an electron…

A

…it becomes positive

53
Q

if an atom gains an electron…

A

…it becomes negative

54
Q

valence level

A

outermost energy level

55
Q

valence electrons

A

electrons in outermost energy level

56
Q

octet rule

A

Atoms bond in such a way to have 8 electrons in their energy levels (hydrogen, helium and lithium are exceptions)

57
Q

covalent bond

A

chemical bond that involves sharing a pair of electrons between atoms in a molecule

58
Q

molecular compound

A

composed of only non-metals

59
Q

chemical reaction

A

a process that occurs when a substance or substances react to form a different substance or substances

60
Q

Biochemical reactions

A
  • cellular respiration (exothermic reaction)
  • photosynthesis (endothermic reaction)
61
Q

Balanced formula equation

A

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
Q

Skeleton formula equation

A

shows which substances are involved but does not show proportions

63
Q

Word equation

A

determine the reactants and products, set up with + and —>
ex: magnesium+hydrochloric acid —> magnesium chloride + hydrogen gas

64
Q

Formation (synthesis)

A

single elements or compounds combine to form larger, more complex compounds

65
Q

Decomposition

A

products are simpler than reactants

66
Q

Hydrocarbon combustion

A

products are always carbon dioxide and water

67
Q

Single replacement

A

cations can only switch with cations, anions can only switch with anions

68
Q

Double replacement

A

exchange of similarly charged ions

69
Q

Mole

A

a quantity that chemists use to measure elements and compounds,
symbol: mol

70
Q

Avogadro’s number

A

the number of atoms or molecules in 1 mol
approximately 6.02 x 10^23,
symbol: NA

71
Q

Molar mass

A

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
Q

How do you find the molar mass of compounds?

A
  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
Q

Molar equation

A

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
Q

How to find “n” in the molar equation formula

A

n= m/M

75
Q

How to find “M” in molar equation formula

A

M= m/n

76
Q

Molar ratio

A

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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