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Chemistry Key Words Flashcards

(55 cards)

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1
Q

Element

A

A substance that cannot be broken down into anything simpler // a substance that is made up of only one type of atom

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2
Q

Atomic Number

A

the number of protons in an atom

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3
Q

Triad

A

elements in groups of 3 with similar chemical and physical properties
the atomic weight of the middle element is halfway between the other 2

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4
Q

Law of Octives

A

every 8th element has similar physical and chemical properties

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5
Q

Matter

A

anything that is made of mass
made up of atoms/molecules/ions

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6
Q

Mass number

A

the sum of protons and neutrons

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7
Q

Isotope

A

the same type of atom
they have the same number of protons but neutrons are different

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8
Q

Relative Atomic Mass (Ar)

A

the average mass of an atom relative to 1/12th of the mass of a carbon 12 isotope

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9
Q

Compound

A

a substance that is made by chemically combining 2 or more elements

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10
Q

Octet Rule

A

when elements combine, they do so to ensure that the outermost shell of electrons of each atom has 8 electrons

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11
Q

Valancy

A

the number of elections that an element needs to lose or gain in order to achieve a noble gas structure

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12
Q

Ionic bonding

A

the transferring of electrons from a metal atom to a non metal atom producing a positive and a negative ion

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13
Q

cation

A

positive ion

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14
Q

anion

A

negative ion

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15
Q

covalent bond

A

the sharing of one or more pairs of electrons between atoms

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16
Q

molecule

A

two or more atoms chemically combined (bonded)

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17
Q

double bond

A

2 pairs of electrons being shared

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18
Q

triple bond

A

3 pairs of electrons being shared

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19
Q

sigma bond

A

a bond that is formed from the head on overlap of orbitals

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20
Q

pi bond

A

a bond formed from the side on overlap of orbitals

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21
Q

polar covalent bonding

A

a covalent bond where the shared pair of electrons is attracted more to one of the joined atoms than to the other

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22
Q

electronegativity

A

the measure of the power of attraction of an atom of that element for the shared pair of electron in a covalent bond

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23
Q

intramolecular bonding

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A

the bonding between the atoms in a molecule

24
Q

intermolecular bonding

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A

the attraction that occurs between different molecules

25
oxidation number
ionic compounds: the oxidation number is the same as the charge on the ion covalent compounds: assume the bond is ionic and the oxidation number is the same as the apparent charge
26
hydrocarbons
compounds that are made up of only carbons and hydrogen atoms
27
saturated
single bonds only
28
homologous series
a family of compounds that have the same functional group they have similar chemical and physical properties successive members differ by CH2
29
unsaturated
doesn’t only have single bonds there are double or triple bonds present
30
polymer
a chain/ large molecule made up of repeating units called monomers
31
aromatic
contains a benzene ring
32
auto-ignition knocking
caused inside an engine when the mixture of petrol and air don’t ignite at the correct time
33
octane number
the measure of the tendency of a fuel to resist knocking
34
avogadros constant
6.02 x 10 power 23
35
a mole
the amount of a substance that contains avogradros constant
36
relative molecular mass (Mr)
the average mass of a molecule relative to 1/12th of the mass of a carbon 12 isotope
37
molar mass
the mass of one mole of a substance (g)
38
molar volume
the volume occupied by one mole of any gas at a definite temperature and pressure
39
ideal gas
a gas that follows all the gas laws under all conditions of temperature and pressure
40
boyles law
for a fixed mass of a gas at a constant temperature, the pressure is inversely proportional to the volume
41
charles law
for a fixed mass of a gas at a constant pressure, the temperature is directly proportional to the volume of
42
gay lussacs law
is all the reactants and the products in a reaction are gases, then the volumes of the gases can be expressed as simple whole numbers
43
avogadros law
equal volumes of all gases at the same temperature and pressure, contain the same number of particles/molecules
44
concentration of a solution
the amount of solute dissolved in a certain amount of solvent
45
standard solution
a solution whose concentration is accurately known
46
primary standards
a substance that is water soluble, stable and available in a pure form it is used to make standard solutions
47
exothermic reactions
reactions that give out heat/energy delta H is negative rise in temp
48
endothermic reactions
reactions that take in heat/energy delta H is positive temperature drop
49
heat of reaction
the heat change when all the moles indicated in the balanced equation react completely
50
bond energy
the energy needed to break one mole of a covalent bond and separate them into neutral atoms
51
heat of combustion
the heat change when one mole of a substance is burned in excess oxygen
52
kilogram calorific volume
the amount of heat generated when one mole of a substance is completely burned
53
heat of formation
the heat change when 1 mole of a substance is formed from its elements in their standard states
54
law of conservation of energy
energy cannot be created or destroyed it is changed from one form to another
55
hess’s law
the heat change for a reaction is the same whether it takes place in one step or a series of steps

chemistry (1 decks)

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