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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
gas to solid =
deposition
26
melting and boiling both require energy how much depends on...
the strength of the forces between the particles
27
the stronger the forces...
the more energy and therefore a higher melting point
28
limitations on diagram:
no forces shown between particles, particles show as inelastic spheres
29
state symbols: solid, liquid, gas, aqueos solution
s,l,g,aq all lowercase
30
atom definition
smallest part of an element that can exist
31
molecule definition
2 or more atoms chemically bonded together
32
compound definition
2 or more diff elements chemically bonded together
33
element definition
a substance that contains only one type of atom
34
carbon dioxide -CO2
35
nitrogen N
36
ammonia NH3
37
chlorine Cl2
38
CO carbon monoxide
39
CH4 methane
40
NaCl sodium chloride`
41
C6H1206 glucouse
42
sulfur dioxide S02
42
sulfur dioxide S02
43
Before electrons were discovered the pre thompson model was that an atom is an invisible sphere
44
Before electrons were discovered the pre thompson model was that an atom is an invisible sphere
45
the discovery of an electron led to Thompson's plum pudding model of an atom
a sphere of positive charge with randomly moving negatively charged electrons
46
rutherford and marsden alpha scattery experiment expectations and reality
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
the nuclear model was developed:
positive nucleus with a mass, cloud of randomly moving negative electrons
48
the bohr model showed electrons orbiting the nucleus in electron shells
49
50
positive protons, neutral neutrons, negative electrons
51
why does the centre of the nucleus have an overall positive charge
it contains positive protons and neutral neutrons
51
why does the centre of the nucleus have an overall positive charge
it contains positive protons and neutral neutrons
52
atoms have a radius of 0.1nm and a nucleus has a radius of 1/10,000th the size of an atom
53
the actual mass and charge of subatomic particles are so small that relative mass and charge are used
go to chem book for table
54
numbers of proton = atomic number
55
number of electrons = number of protons
56
the overall charge on an atom is neutral because there is the same number of positive protons as negative electrons
57
number of neutrons = mass number - atomic number
58
relative mass definition
the average atomic mass of all isotopes present in percentage
59
relative mass definition
the average atomic mass of all isotopes present in percentage
60
absolute mass definition
sum of numbers of protons and neutrons mass
61
electrons orbit the nucleus in shells
62
each shell is fully filled before moving on to the next the rule is called 2.8.8.18 rule
63
isotope definition
an atom of an element that has the same number or protons but a diff number of neutrons

year 9 chem eoy (7 decks)

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