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A Level Chemistry > module 2 atoms and reactions > Flashcards

module 2 atoms and reactions Flashcards

1
Q

What is the formula for carbon dioxide

A

CO2

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2
Q

what is the formula for carbon monoxide

A

CO

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3
Q

what is the formula for nitrogen monoxide

A

NO

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4
Q

what is the formula for sulfur trioxide

A

SO3

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5
Q

what is the formula for ammonia

A

NH3

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6
Q

what is the formula for methane

A

CH4

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7
Q

what is the formula for hydrogen sulfide

A

H2S

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8
Q

what is the formula for hydrogen

A

H2

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9
Q

What is the formula for nitrogen

A

N2

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10
Q

what is the formula for oxygen

A

O2

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11
Q

what is the formula for fluorine

A

F2

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12
Q

what is the formula for phosphorus

A

P4

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13
Q

what is the formula for sulfur

A

S8

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14
Q

what is the formula for hydrochloric acid

A

HCl

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15
Q

what is the formula for sulfuric acid

A

H2SO4

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16
Q

what is the formula for nitric acid

A

HNO3

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17
Q

what is the formula for phosphoric acid

A

H3PO4

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18
Q

What is the charge on a group 1 ion

A

+

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19
Q

What is the charge on a group 2 ion

A

2+

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20
Q

What is the charge on a group 3 ion

A

3+

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21
Q

what is the ion of ammonium

A

NH4^+

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22
Q

what is the charge of a group 7 ion

A

-

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23
Q

what is the charge of group 6 ions

24
Q

what is the formula for a nitrate ion

25
Q

what is the formula of a sulfate ion

26
Q

what is the formula of a carbonate ion

27
Q

what is the formula of a hydrogencarbonate ion

28
Q

what is the formula of a hydroxide ion

29
Q

what is the formula for a hydride ion

30
Q

what is the formula for a phosphate ion

31
Q

acid + metal ->

A

salt + hydrogen

32
Q

acid + metal oxide ->

A

salt + water

33
Q

acid + carbonate ->

A

salt + water + carbon dioxide

34
Q

acid + hydroxide ->

A

salt + water

35
Q

hydrocarbon + oxygen ->

A

carbon dioxide + water

36
Q

acid + ammonia ->

A

ammonium salt

37
Q

What is the electron configuration for krypton (the furthest you can be asked to go - can work out others from this one)

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6

38
Q

what is an orbital

A

a bit of space that an electron moves in

39
Q

if there are 2 electrons in an orbital, which direction will they spin

A

opposite directions

40
Q

what shape are S orbitals

41
Q

what shape are p orbitals

A

dumbbell shaped

42
Q

what is a precipitate

A

the insoluble product when 2 solutions are mixed

43
Q

can we have a nitrate precipitate and if so which ones

A

no as all nitrates are soluble

44
Q

can we have a halide precipitate and if so which ones

A

most halides are soluble so wouldn’t form a precipitate however silver halides and lead halides would form a precipitate

45
Q

can we form sulfate precipitates and if so which ones

A

most sulfates are soluble so wouldn’t but lead sulfate, barium sulfate and calcium sulfate would

46
Q

can we form a carbonate precipitate and if so which ones

A

most carbonates produce a precipitate and the only ones that don’t are lithium carbonate, sodium carbonate, potassium carbonate and ammonium carbonate

47
Q

can a hydroxide form a precipitate

A

most hydroxides will form a precipitate however lithium hydroxide, sodium hydroxide, potassium hydroxide, ammonium hydroxide and group 2 hydroxides

48
Q

Describe the relative energies of the 2s orbital and each of the three 2p orbitals in a nitrogen atom

A
  • p orbitals have greater energy than s orbitals
  • the 3 p orbitals have equal energy
49
Q

How many electrons can be in each of the first 4 shells

A

1st = 2
2nd = 8
3rd = 18
4th = 32

50
Q

What did Dalton believe the atom was in 1803

A

Solid sphere with no subatomic particles

51
Q

What did Thompson believe the atom was in 1897

A

Plum pudding model - mass of positive with negative wedged in

52
Q

What did Rutherford believe the atom was in 1909

A

Mass mainly positive in centre (nucleus) but there is empty space

53
Q

How did Bohr develop the atom in 1913

A

Added that electrons orbited in shells / energy levels

54
Q

What does the current atom (nuclear model) look like

A

Protons and neutrons making up the nucleus with mainly empty space and electrons orbiting in shells

55
Q

Define relative atomic mass

A

Weighted mean mass of an atom of an element compared to 1/12th the mass of an atom of carbon 12 which is taken as exactly 12. It is a weighted mean due to the presence of isotopes.

56
Q

Define relative isotopic mass

A

Mass of an atom of an isotope of an element compared to 1/12th the mass of an atom of carbon 12 which is taken as exactly 12

57
Q

How do you calculate relative atomic mass

A

(Atomic number x percentage as a decimal) + (Atomic number x percentage as a decimal)

A Level Chemistry (3 decks)

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