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year 9 chem eoy > funamentals > Flashcards

funamentals Flashcards

1
Q

sulfuric acid formula and salt ending

A

H₂SO₄, sulfate

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2
Q

hydrochloric acid formula and salt ending

A

HCl, chloride

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3
Q

ethanoic acid formula and salt ending

A

CH₃COOH, ethanoate

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4
Q

nitric acid formula and salt ending

A

HNO₃ nitrate

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5
Q

acid definition

A

a substance that releases H+ ions in water (pH<7)

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6
Q

base definition

A

a substance that reacts with an acid to form a salt

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7
Q

bases examples

A

cc

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8
Q

alkali definition

A

a soluble base (pH>7)

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9
Q

indicator definition

A

a chemical that changes colour depending on whether its an acid or alkali

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10
Q

general equation for metal oxide + acid

A

metal oxide + acid -> salt + water

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11
Q

when reacting a metal oxide with an acid why will it not produce an alkali solution

A

when reacting a metal oxide with an acid it will not produce an alkali solution due to the excess metal oxide not reacting

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12
Q

general equation : metal + acid -> salt + hydrogen (MASH)

A
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13
Q

test for hydrogen

A

lit splint burns with a squeaky pop

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14
Q

general equation: metal carbonate + acid ->

A

general equation: metal carbonate + acid -> salt + water + carbon dioxide

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15
Q

test for carbon dioxide

A

limewater turns cloudy

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16
Q

general equation: metal hydroxide + acid ->

A

general equation: metal hydroxide + acid -> salt + water

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17
Q

colour and strength, pH1-2, 3-4, 5-6, 7, 8-10, 11-14

A

1-2 strong ,red, 3-4 weak, orange, 5-6 acid, yellow, 7 neutral ,green, 8-10 weak alkali, blue,11-14 strong alkali, purple

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18
Q

what is the pH scale a measure of

A

the pH scale is a measure of how acidic a substance is. Strong acids react more vigorously than weak acids

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19
Q

what is universal indicator

A

universal indicator is a mixture of many different indicators, the mixture gives universal indicator a wide range of colours most indicators have 2 or 3 diff colours but do not all change at exactly pH7. this means they will have 1 colour below a specific pH and a diff colour above that pH

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20
Q

solid to gas =

A

sublimation

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21
Q

solid to liquid = melting

A
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22
Q

liquid to solid =

A

freezing

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23
Q

liquid to gas

A

evaporating

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24
Q

gas to liquid =

A

condensation

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25
Q

gas to solid =

A

deposition

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26
Q

melting and boiling both require energy how much depends on…

A

the strength of the forces between the particles

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27
Q

the stronger the forces…

A

the more energy and therefore a higher melting point

28
Q

limitations on diagram:

A

no forces shown between particles, particles show as inelastic spheres

29
Q

state symbols: solid, liquid, gas, aqueos solution

A

s,l,g,aq all lowercase

30
Q

atom definition

A

smallest part of an element that can exist

31
Q

molecule definition

A

2 or more atoms chemically bonded together

32
Q

compound definition

A

2 or more diff elements chemically bonded together

33
Q

element definition

A

a substance that contains only one type of atom

34
Q

carbon dioxide -CO2

A
35
Q

nitrogen N

A
36
Q

ammonia NH3

A
37
Q

chlorine Cl2

A
38
Q

CO carbon monoxide

A
39
Q

CH4 methane

A
40
Q

NaCl sodium chloride`

A
41
Q

C6H1206 glucouse

A
42
Q

sulfur dioxide S02

A
42
Q

sulfur dioxide S02

A
43
Q

Before electrons were discovered the pre thompson model was that an atom is an invisible sphere

A
44
Q

Before electrons were discovered the pre thompson model was that an atom is an invisible sphere

A
45
Q

the discovery of an electron led to Thompson’s plum pudding model of an atom

A

a sphere of positive charge with randomly moving negatively charged electrons

46
Q

rutherford and marsden alpha scattery experiment expectations and reality

A

positive alpha particles fired at gold atoms should be deflected evenly by positive spheres however most α particles went through showing that most of the atom is empty space, some particles were deflected at extreme angles showing that the centre was positively charged and has a mass

47
Q

the nuclear model was developed:

A

positive nucleus with a mass, cloud of randomly moving negative electrons

48
Q

the bohr model showed electrons orbiting the nucleus in electron shells

A
49
Q
A
50
Q

positive protons, neutral neutrons, negative electrons

A
51
Q

why does the centre of the nucleus have an overall positive charge

A

it contains positive protons and neutral neutrons

51
Q

why does the centre of the nucleus have an overall positive charge

A

it contains positive protons and neutral neutrons

52
Q

atoms have a radius of 0.1nm and a nucleus has a radius of 1/10,000th the size of an atom

A
53
Q

the actual mass and charge of subatomic particles are so small that relative mass and charge are used

A

go to chem book for table

54
Q

numbers of proton = atomic number

A
55
Q

number of electrons = number of protons

A
56
Q

the overall charge on an atom is neutral because there is the same number of positive protons as negative electrons

A
57
Q

number of neutrons = mass number - atomic number

A
58
Q

relative mass definition

A

the average atomic mass of all isotopes present in percentage

59
Q

relative mass definition

A

the average atomic mass of all isotopes present in percentage

60
Q

absolute mass definition

A

sum of numbers of protons and neutrons mass

61
Q

electrons orbit the nucleus in shells

A
62
Q

each shell is fully filled before moving on to the next the rule is called 2.8.8.18 rule

A
63
Q

isotope definition

A

an atom of an element that has the same number or protons but a diff number of neutrons

year 9 chem eoy (6 decks)

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