Chemistry 10 review Flashcards
(119 cards)
1
Q
Matter
A
anything that has mass and volume
2
Q
Pure substances
A
cannot be broken down into any other substances
3
Q
Compounds
A
combination of 2 or more elements
4
Q
elements
A
composed of only one type of atom
5
Q
Mixture
A
combination of 2 or more compounds
6
Q
Heterogeneous mixtures
A
contains 2 or more substances with VISIBLE parts
7
Q
Colloid
A
cannot be easily separated, cloudy mixture. LIQUID IN LIQUID
ex: milk
8
Q
Suspension
A
can be easily separated. SOLID IN LIQUID
ex: mud (water+soil)
9
Q
Mechanical mixture
A
different substances are visible
ex: salad
10
Q
Homogenous mixture (solution)
A
all substances are uniform throughout and there’s no distinctive visible parts. Appears to be 1
11
Q
Properties
A
characteristics used to describe a substance
12
Q
Physical properties
A
observable physical characteristics of a substance.
ex: boiling/melting points, conductivity, malleability, ductility, state, solubility, melting/freezing point
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)
14
Q
Chemical change
A
new substances are formed after chemical reactions. Chemical components CHANGE
ex: change in temperature, precipitate, light, odour, colour
15
Q
Chemical reactions
A
one or more substance react to form new substance(s)
16
Q
Indicators of chemical change
A
energy flow, formation of gas, precipitate, formation of new substances w/ different properties
17
Q
Atom
A
smallest part of an element. NEUTRAL. has protons, neutrons, electrons.
ex: oxygen atom
18
Q
Subatomic particles
A
particles that make up an atom. PROTONS, NEUTRONS, ELECTRONS
19
Q
Protons
A
(+) charged particles, atomic number, found in nucleus, heavy, never change
20
Q
Neutrons
A
no charge, belongs to nucleus, heavy, can change (isotope)
21
Q
Electrons
A
(-) charge particles, no mass, found in electron cloud/energy levels, can change (ion)
22
Q
Nucleons
A
Particles found in the nucleus: protons and neutrons
23
Q
Metals
A
elements on the left side of staircase, cations, (+) charge, give away electrons
24
Q
Metal properties
A
Ductile, malleable, conductive, shiny, hard, reactive
25
Malleable
ability to be rolled into sheets
26
Ductile
ability to be stretched into wires
27
Non metals
elements on the right side of staircase, (-) charge, anions, receive electrons
ex: O-oxygen
28
Non metal properties
Non-magnetic, brittle, not shiny, poor conductors, non-malleable, low melting/boiling points
29
Inert
Substances that are chemically unreactive
| ex: noble gases
30
Metalloid
Group 13-16 along staircase, have properties between metals and non-metals, semi-conductors
31
Period
horizontal rows, indicates number of energy levels
| ex: Na - period 2 —> 2 energy levels
32
Group/Family
vertical columns, elements in each group have same number of valence electrons, similar properties,
33
Group 1
ALKALI METALS. highly reactive, conductive, soluble, 1 valence electron, shiny, silvery, charge of +1, low melting/boiling points
34
Group 2
ALKALINE EARTH METALS. less reactive, 2 valence electrons, silvery white, soluble, low melting/boiling points
35
Group 3-12
TRANSITION METALS. conductive, high melting/boiling points, malleable, ductile, high densities
36
Group 13-16
METALLOIDS. properties between metals and non-metals, poor conductors, solid, metallic lustre
37
Group 17
HALOGENS. 7 valence electrons, highly reactive
38
Group 18
NOBLE GASES. non-reactive, full valence shell, odourless, colourless, non-flammable
39
Energy levels
orbitals occupied by electrons
CLOSEST to nucleus- LOWEST ENERGY
FURTHER away- HIGHER energy
40
Valence shell
outermost shell. determine an atom's reactivity
41
Atomic number
of PROTONS, ELECTRONS
42
Atomic mass
average mass of an atom, PROTONS + NEUTRONS
43
Isotopes
the same element with a different number of neutrons resulting the MASS CHANGE, same chemically
44
Ionization
the process of gaining/losing electrons
45
Ion
when an atom gains or loses its electron(s), has an electrical charge
46
Cation
metals, + charge, loses electrons
47
Anion
non-metals, - charge, gains electrons
48
Valence electrons
electrons in the outermost shell, involves in chemical bonds
49
Valence number
number of electrons that can be given up or received by another ion
50
Octet Rule
atoms bond in a way to achieve 8 electrons in its valence shell to achieve stability like its nearest noble gas (full valence)
51
Octet rule exception
H, Be, Li. only need 2 valence electrons like its nearest noble gas Helium
52
Ionic bond
formed metal and non-metal. TRANSFER OF ELECTRONS. form ionic compounds
53
Ionic compounds
formed when electrons are transferred between a metal and a non-metal
54
Ionic Compound properties
cation+anion, transfer of e-, crystal shape, high melting/boiling points, soluble, conductive, form precipitate, solid at room temp.
55
Crystal Lattice
array of points repeating in 3-D, creates crystal shapes of an element
56
Fomula Unit
ratio of cation to anion in ionic/molecular compounds
57
Multivalent
element that has more than one charge, ROMAN NUMERALS
58
Polyatomic ions
2 or more nonmetals combined to form a (-) charged ion
59
Molecular compound
when electrons are shared between 2 non-metals
60
Molecular compound properties
e- shared b/w 2 ions, covalent bond, low melting/boiling points, insoluble, non-conductive, no precipitate
61
Molecular:
LARGER MOLECULES
solid
62
Molecular
SMALLER MOLECULES
gas
63
Covalent bond
when e- are shared between 2 non-metals ions
64
Molecular element
molecules with only ONE type of atom
65
Polyatomic
more than 2 of the same atom bonded together
| ex: S8, P4
66
Polar
compounds that have a charge difference, positive end and negative end. Unequal sharing of electrons in hydrogen toms
ex: Water
67
Conductivity
The ability to conduct or carry an electrical current
| ex: metals
68
Diatomic element
atoms of the same element bond in PAIRS to form molecules
| ex: O2
69
Electrolyte
conduction chemical solution
70
Solubility
the ability to dissolve in water
71
Slightly soluble
solid
72
Very soluble
aqueous
73
Precipitation
formation of a solid in an IONIC chemical reaction. appears as white, cloudy substance
74
Acid
pH < 7, always AQUEOUS, hydrogen ions
75
Acid properties
sour, corrodes metals, conductive, litmus red, neutralize bases, produce H2 gas
76
Base
pH > 7, can be AQUEOUS/SOLID, OH- ions
77
Base properties
conductive, bitter, litmus blue, dissolves grease, do not react w/ metals, neutralize acids
78
Neutral
pH = 7
79
Indicator
tools used to indicate whether a substance is an acid or base
ex: litmus paper
80
Neutralization
chemical reactions that form salts and water. Combing an acid and a base to bring pH = 7
81
Base neutralization
add acid
82
Acid neutralization
add base
83
Salt
ionic compound produced by a neutralization reaction
84
Reactants
starting materials before chemical reaction
85
Products
new substances after chemical reaction
86
Antoine Lavoisier
proposed the law of conservation of mass
87
Law of conservation of mass
mass of reactants = mass of products
88
Exothermic
a chemical reaction that releases energy in form of heat, light, electricity
ex: cellular respiration (reversed process of photosynthesis)
89
Endothermic
a chemical reaction that requires energy or absorbs energy.
| ex: photosynthesis
90
Chemical equation
using symbols/formulas to represent a chemical reaction
| INCLUDES balancing
91
Skeleton equation
using symbols/formulas to represent a chemical reaction
| NO BALANCING
92
Balanced equation
include balancing
93
Formation/Synthesis/Simple composition
when 2 or more elements are combined to form an ionic/molecular compound
94
Simple decomposition
when an ionic/molecular compound is broken down into its elements
95
Single replacement
when an element react with an ionic compound to form a new element and new ionic compound
96
Double replacement
when 2 ionic compounds react to form 2 new ionic compounds
97
Hydrocarbon combustion
when a hydrocarbon compound reacts with O2 to produce CO2 and water
98
Mole
6.02 x 10^23 of something. How much of substance is present
99
Avagadro's constant
6.02 x10^23
100
Molar Mass
mass in grams of one mole of a substance
| g/mol
101
Billiard Ball Model
John Dalton: all atoms were like small spheres with different properties that varied in size, mass, and colour
102
Plum-pudding model
J.J Thomson: discovered ELECTRONS. atom was a sphere was (+) charge particles with (-) particles floating WITHIN it
103
Ernest Rutherford
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
Neil Bohr
Electrons surround the nucleus in specific ENERGY LEVELS
105
Quantum Mechanics
electrons occupy the whole space all at once with different energy levels as a cloud (opposite of Bohr Model)
Marker experiment
106
Dmitri Mendeleev
constructed the 1st period table
107
Hydrogen element
non-metal, behave like an alkali metal and have similar properties as alkali metals
108
Democritus
all matter was made up of tiny particles that are INDESTRUCTIBLE & INDIVISIBLE
109
High electron cloud density (orbital)
high probability of finding electrons
110
Low electron cloud density
low probability of finding electrons
111
Buffer
substance that keeps pH constant even when small amounts of acid/base is added
112
pH scale (increase)
every increase of 1 indicates increase of 10 as pH increases (increase alkalinity)
113
pH scale decrease
every decrease of 1 indicates decrease of 10 as pH decreases (increase acidity)
114
Naming acid
hydrogen + non-metal
hydro__ic acid
115
Naming acid
hydrogen + polyatomic ATE
__ic acid
116
Naming acid
hydrogen + polyatomic ITE
__ous acid
117
Naming base
__hydroxide
118
Ice
less dense than water, lighter (lower mass), water freezes molecules expand
119
Aristotle
all matter was composed of fire, earth, water, air
