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Chemistry 10 > Chemistry 10 review > Flashcards

Chemistry 10 review Flashcards

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1
Q

Matter

A

anything that has mass and volume

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2
Q

Pure substances

A

cannot be broken down into any other substances

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3
Q

Compounds

A

combination of 2 or more elements

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4
Q

elements

A

composed of only one type of atom

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5
Q

Mixture

A

combination of 2 or more compounds

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6
Q

Heterogeneous mixtures

A

contains 2 or more substances with VISIBLE parts

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7
Q

Colloid

A

cannot be easily separated, cloudy mixture. LIQUID IN LIQUID

ex: milk

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8
Q

Suspension

A

can be easily separated. SOLID IN LIQUID

ex: mud (water+soil)

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9
Q

Mechanical mixture

A

different substances are visible

ex: salad

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10
Q

Homogenous mixture (solution)

A

all substances are uniform throughout and there’s no distinctive visible parts. Appears to be 1

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11
Q

Properties

A

characteristics used to describe a substance

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12
Q

Physical properties

A

observable physical characteristics of a substance.

ex: boiling/melting points, conductivity, malleability, ductility, state, solubility, melting/freezing point

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13
Q

Chemical properties

A

how a substance reacts with other substances

ex: reaction with acid/water/air/heat, litmus paper, ability to burn, temperature to ignite a flame (flash point)

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14
Q

Chemical change

A

new substances are formed after chemical reactions. Chemical components CHANGE
ex: change in temperature, precipitate, light, odour, colour

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15
Q

Chemical reactions

A

one or more substance react to form new substance(s)

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16
Q

Indicators of chemical change

A

energy flow, formation of gas, precipitate, formation of new substances w/ different properties

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17
Q

Atom

A

smallest part of an element. NEUTRAL. has protons, neutrons, electrons.
ex: oxygen atom

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18
Q

Subatomic particles

A

particles that make up an atom. PROTONS, NEUTRONS, ELECTRONS

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19
Q

Protons

A

(+) charged particles, atomic number, found in nucleus, heavy, never change

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20
Q

Neutrons

A

no charge, belongs to nucleus, heavy, can change (isotope)

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21
Q

Electrons

A

(-) charge particles, no mass, found in electron cloud/energy levels, can change (ion)

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22
Q

Nucleons

A

Particles found in the nucleus: protons and neutrons

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23
Q

Metals

A

elements on the left side of staircase, cations, (+) charge, give away electrons

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24
Q

Metal properties

A

Ductile, malleable, conductive, shiny, hard, reactive

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25
Q

Malleable

A

ability to be rolled into sheets

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26
Q

Ductile

A

ability to be stretched into wires

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27
Q

Non metals

A

elements on the right side of staircase, (-) charge, anions, receive electrons
ex: O-oxygen

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28
Q

Non metal properties

A

Non-magnetic, brittle, not shiny, poor conductors, non-malleable, low melting/boiling points

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29
Q

Inert

A

Substances that are chemically unreactive

ex: noble gases

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30
Q

Metalloid

A

Group 13-16 along staircase, have properties between metals and non-metals, semi-conductors

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31
Q

Period

A

horizontal rows, indicates number of energy levels

ex: Na - period 2 —> 2 energy levels

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32
Q

Group/Family

A

vertical columns, elements in each group have same number of valence electrons, similar properties,

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33
Q

Group 1

A

ALKALI METALS. highly reactive, conductive, soluble, 1 valence electron, shiny, silvery, charge of +1, low melting/boiling points

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34
Q

Group 2

A

ALKALINE EARTH METALS. less reactive, 2 valence electrons, silvery white, soluble, low melting/boiling points

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35
Q

Group 3-12

A

TRANSITION METALS. conductive, high melting/boiling points, malleable, ductile, high densities

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36
Q

Group 13-16

A

METALLOIDS. properties between metals and non-metals, poor conductors, solid, metallic lustre

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37
Q

Group 17

A

HALOGENS. 7 valence electrons, highly reactive

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38
Q

Group 18

A

NOBLE GASES. non-reactive, full valence shell, odourless, colourless, non-flammable

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39
Q

Energy levels

A

orbitals occupied by electrons
CLOSEST to nucleus- LOWEST ENERGY
FURTHER away- HIGHER energy

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40
Q

Valence shell

A

outermost shell. determine an atom’s reactivity

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41
Q

Atomic number

A

of PROTONS, ELECTRONS

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42
Q

Atomic mass

A

average mass of an atom, PROTONS + NEUTRONS

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43
Q

Isotopes

A

the same element with a different number of neutrons resulting the MASS CHANGE, same chemically

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44
Q

Ionization

A

the process of gaining/losing electrons

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45
Q

Ion

A

when an atom gains or loses its electron(s), has an electrical charge

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46
Q

Cation

A

metals, + charge, loses electrons

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47
Q

Anion

A

non-metals, - charge, gains electrons

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48
Q

Valence electrons

A

electrons in the outermost shell, involves in chemical bonds

49
Q

Valence number

A

number of electrons that can be given up or received by another ion

50
Q

Octet Rule

A

atoms bond in a way to achieve 8 electrons in its valence shell to achieve stability like its nearest noble gas (full valence)

51
Q

Octet rule exception

A

H, Be, Li. only need 2 valence electrons like its nearest noble gas Helium

52
Q

Ionic bond

A

formed metal and non-metal. TRANSFER OF ELECTRONS. form ionic compounds

53
Q

Ionic compounds

A

formed when electrons are transferred between a metal and a non-metal

54
Q

Ionic Compound properties

A

cation+anion, transfer of e-, crystal shape, high melting/boiling points, soluble, conductive, form precipitate, solid at room temp.

55
Q

Crystal Lattice

A

array of points repeating in 3-D, creates crystal shapes of an element

56
Q

Fomula Unit

A

ratio of cation to anion in ionic/molecular compounds

57
Q

Multivalent

A

element that has more than one charge, ROMAN NUMERALS

58
Q

Polyatomic ions

A

2 or more nonmetals combined to form a (-) charged ion

59
Q

Molecular compound

A

when electrons are shared between 2 non-metals

60
Q

Molecular compound properties

A

e- shared b/w 2 ions, covalent bond, low melting/boiling points, insoluble, non-conductive, no precipitate

61
Q

Molecular:

LARGER MOLECULES

A

solid

62
Q

Molecular

SMALLER MOLECULES

A

gas

63
Q

Covalent bond

A

when e- are shared between 2 non-metals ions

64
Q

Molecular element

A

molecules with only ONE type of atom

65
Q

Polyatomic

A

more than 2 of the same atom bonded together

ex: S8, P4

66
Q

Polar

A

compounds that have a charge difference, positive end and negative end. Unequal sharing of electrons in hydrogen toms
ex: Water

67
Q

Conductivity

A

The ability to conduct or carry an electrical current

ex: metals

68
Q

Diatomic element

A

atoms of the same element bond in PAIRS to form molecules

ex: O2

69
Q

Electrolyte

A

conduction chemical solution

70
Q

Solubility

A

the ability to dissolve in water

71
Q

Slightly soluble

A

solid

72
Q

Very soluble

A

aqueous

73
Q

Precipitation

A

formation of a solid in an IONIC chemical reaction. appears as white, cloudy substance

74
Q

Acid

A

pH < 7, always AQUEOUS, hydrogen ions

75
Q

Acid properties

A

sour, corrodes metals, conductive, litmus red, neutralize bases, produce H2 gas

76
Q

Base

A

pH > 7, can be AQUEOUS/SOLID, OH- ions

77
Q

Base properties

A

conductive, bitter, litmus blue, dissolves grease, do not react w/ metals, neutralize acids

78
Q

Neutral

A

pH = 7

79
Q

Indicator

A

tools used to indicate whether a substance is an acid or base
ex: litmus paper

80
Q

Neutralization

A

chemical reactions that form salts and water. Combing an acid and a base to bring pH = 7

81
Q

Base neutralization

A

add acid

82
Q

Acid neutralization

A

add base

83
Q

Salt

A

ionic compound produced by a neutralization reaction

84
Q

Reactants

A

starting materials before chemical reaction

85
Q

Products

A

new substances after chemical reaction

86
Q

Antoine Lavoisier

A

proposed the law of conservation of mass

87
Q

Law of conservation of mass

A

mass of reactants = mass of products

88
Q

Exothermic

A

a chemical reaction that releases energy in form of heat, light, electricity
ex: cellular respiration (reversed process of photosynthesis)

89
Q

Endothermic

A

a chemical reaction that requires energy or absorbs energy.

ex: photosynthesis

90
Q

Chemical equation

A

using symbols/formulas to represent a chemical reaction

INCLUDES balancing

91
Q

Skeleton equation

A

using symbols/formulas to represent a chemical reaction

NO BALANCING

92
Q

Balanced equation

A

include balancing

93
Q

Formation/Synthesis/Simple composition

A

when 2 or more elements are combined to form an ionic/molecular compound

94
Q

Simple decomposition

A

when an ionic/molecular compound is broken down into its elements

95
Q

Single replacement

A

when an element react with an ionic compound to form a new element and new ionic compound

96
Q

Double replacement

A

when 2 ionic compounds react to form 2 new ionic compounds

97
Q

Hydrocarbon combustion

A

when a hydrocarbon compound reacts with O2 to produce CO2 and water

98
Q

Mole

A

6.02 x 10^23 of something. How much of substance is present

99
Q

Avagadro’s constant

A

6.02 x10^23

100
Q

Molar Mass

A

mass in grams of one mole of a substance

g/mol

101
Q

Billiard Ball Model

A

John Dalton: all atoms were like small spheres with different properties that varied in size, mass, and colour

102
Q

Plum-pudding model

A

J.J Thomson: discovered ELECTRONS. atom was a sphere was (+) charge particles with (-) particles floating WITHIN it

103
Q

Ernest Rutherford

A

discovered NUCLEUS. nucleus was like an ant in a football field. Atoms contains mostly empty spaces with a (+) nucleus consisted of (+) charged particles with (-) charged particles ORBITING it

104
Q

Neil Bohr

A

Electrons surround the nucleus in specific ENERGY LEVELS

105
Q

Quantum Mechanics

A

electrons occupy the whole space all at once with different energy levels as a cloud (opposite of Bohr Model)

Marker experiment

106
Q

Dmitri Mendeleev

A

constructed the 1st period table

107
Q

Hydrogen element

A

non-metal, behave like an alkali metal and have similar properties as alkali metals

108
Q

Democritus

A

all matter was made up of tiny particles that are INDESTRUCTIBLE & INDIVISIBLE

109
Q

High electron cloud density (orbital)

A

high probability of finding electrons

110
Q

Low electron cloud density

A

low probability of finding electrons

111
Q

Buffer

A

substance that keeps pH constant even when small amounts of acid/base is added

112
Q

pH scale (increase)

A

every increase of 1 indicates increase of 10 as pH increases (increase alkalinity)

113
Q

pH scale decrease

A

every decrease of 1 indicates decrease of 10 as pH decreases (increase acidity)

114
Q

Naming acid

hydrogen + non-metal

A

hydro__ic acid

115
Q

Naming acid

hydrogen + polyatomic ATE

A

__ic acid

116
Q

Naming acid

hydrogen + polyatomic ITE

A

__ous acid

117
Q

Naming base

A

__hydroxide

118
Q

Ice

A

less dense than water, lighter (lower mass), water freezes molecules expand

119
Q

Aristotle

A

all matter was composed of fire, earth, water, air

Chemistry 10 (1 decks)

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