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CH 1 > Introduction to CH1 > Flashcards

Introduction to CH1 Flashcards

0
Q

What does the mass number of an element tell you?

A

The number of protons and neutrons in an atom of the element.

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1
Q

What does the atomic number of an element tell you?

A

The number of protons one atom has in an element

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2
Q

How can you work out the number of electrons in a stable atom?

A

The number of protons will be the same to give it a neutral charge.

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3
Q

What is the lithium ion?

A

Li+1

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4
Q

What is the charge of sodium?

A

+1

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5
Q

What is the potassium ion?

A

K+1

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6
Q

What is the charge of silver?

A

+1

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7
Q

What is the charge of copper(I)?

A

+1

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8
Q

What is the ion of ammonium?

A

(NH4)+1

Note: there’s no subscript so the formula is in the bracket)

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9
Q

What is the ion of hydrogen?

A

H+1

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10
Q

What is the charge of mercury?

A

+1

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11
Q

What is the charge of beryllium?

A

+2

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12
Q

What’s the ion of magnesium?

A

Mg+2

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13
Q

What’s the charge of calcium?

A

+2

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14
Q

What is the ion of copper(II)?

A

Cu+2

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15
Q

What is the charge of zinc?

A

+2

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16
Q

What’s the ion of lead(II)?

A

Pb+2

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17
Q

What’s the charge of barium?

A

+2

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18
Q

What’s the ion of manganese(II)?

A

Mn+2

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19
Q

What’s the ion of iron(II)?

A

Fe+2

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20
Q

What’s the charge of iron(III)?

A

Fe+3

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21
Q

What’s the ion of aluminium?

A

Al+3

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22
Q

What’s the charge of chromium(III)?

A

+3

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23
Q

What’s the charge of Lead(IV)?

A

+4

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24
Q

What’s the ion of manganese(IV)?

A

Mn+4

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25
Q

What’s the ion of vanadium(V)?

A

+5

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26
Q

What’s the ion if chromium(VI)?

A

Cr+6

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27
Q

What’s the charge of fluoride?

A

F-1

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28
Q

What’s the ion of chlorine?

A

Chloride/Cl-1

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29
Q

What’s the charge of bromide?

A

-1

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30
Q

What’s the ion of iodine?

A

Iodide/I-1

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31
Q

What’s the ion of nitrite?

A

(NO2)-1

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32
Q

What’s the ion of nitrate?

A

(NO3)-1

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33
Q

What’s the ion of hydrogencarbonate?

A

(HCO3)-1

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34
Q

What’s the ion of hydrogensulfate?

A

(HSO4)-1

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35
Q

What’s the ion of hydroxide?

A

OH-1

36
Q

What’s the ion of oxide?

A

O-2

37
Q

What’s the ion of sulphide?

A

S-2

38
Q

What’s the ion of sulphite?

A

(SO3)-2

39
Q

What’s the ion of Sulphate?

A

(SO4)-2

40
Q

What’s the ion of Carbonate?

A

(CO3)-2

41
Q

What’s the ion of nitride?

A

N-3

42
Q

What’s the ion of phosphide?

A

P-3

43
Q

What’s the ion of phosphate?

A

(PO4)-3

44
Q

What’s the ion of carbide?

A

C-4

45
Q

What’s the ion of silicide?

A

Si-4

46
Q

Name 4 elements with varying valencies.

A

Copper
Iron
Manganese
Chromium

47
Q

Name 7 diatomic elements

A

Nitrogen, oxygen, hydrogen, iodine, chlorine, fluorine and bromine.

48
Q

What do half equations show?

A

Whats happening to each ion in a reaction, only one half, one element’s reaction, is shown.

49
Q

What is the overall and half equations for the reaction of sodium and chloride?

A

2Na + Cl2 (arrow) 2NaCl
Na - e- (arrow) Na+1
Cl2 - 2e- (arrow) 2Cl-1

50
Q

What will a reaction between an acid and a base ALWAYS produce?

A

Salt and Water

51
Q

Write and solve a combustion equation for the combustion of propane.

A

C3H8 + 5O2 (arrow) 3CO2 + 3H2O

52
Q

What is the maximum number of electrons that can be in the first shell of an element?

A

2

53
Q

What is the maximum number of electrons that can be in the second shell of an element?

A

8

54
Q

What is the maximum number of electrons that can be in the third shell of an element?

A

18

55
Q

What is it called when an element loses electrons?

A

Oxidation.

56
Q

What is it called when an element gains electrons?

A

Reduction.

57
Q

What is ionic bonding?

A

When elements react together by gaining or losing electrons.

58
Q

What is covalent bonding?

A

When elements share electrons.

59
Q

What bonding occurs when sodium chloride is produced?

A

Ionic bonding.

60
Q

What bonding occurs when hydrogen chloride is produced?

A

Covalent bonding.

61
Q

What is the definition of coordinate (dative) bonding?

A

It’s a covalent bond where both bonding electrons come from only one atom.

62
Q

What shape is the S- orbital described as?

A

A circle

63
Q

What shape is the P- orbital described as?

A

A figure of 8

64
Q

How many electron pairs can go in a s- orbital?

A

1

65
Q

How many electron pairs can go in a p- orbital?

A

3

66
Q

How many electron pairs can go in a d- orbital?

A

5

68
Q

What is Hund’s rule?

A

That every electron must be put into a vacant orbital so that it’s unpaired. Only pair up electrons when there is no vacant orbital.

69
Q

What are the two special cases in the electronic configuration of the first 36 elements? How are they different from all the other elements?

A

Chromium and copper, because one of the paired electrons in the 4S orbital of chromium atom goes as a lone electron in the 3d orbital to make it more stable. In the copper atom one of the paired 4S electrons go to pair up in the 3d orbital, to make it more stable.

70
Q

What is the electric configuration of Neon

A

(1S)2, (2S)2, (2P)6

71
Q

What is the electric configuration of Chlorine?

A

(1S)2, (2S)2, (2P)6, (3S)2, (3P)5

72
Q

What is the electric configuration of chromium?

A

(1S)2, (2S)2, (2P)6, (3S)2, (3P)6, (4S)1, (3D)5

73
Q

What is the electric configuration of copper?

A

(1S)2, (2S)2, (2P)6, (3S)2, (3P)6, (4S)1, (3D)10

74
Q

What is the electric configuration of iron?

A

(1S)2, (2S)2, (2P)6, (3S)2, (3P)6, (4S)2, (3D)6

75
Q

How do you write electric configuration in short hand?

A

By using a noble gas structure for the first couple of orbitals as they are always full.

76
Q

Write the electric configuration of calcium in shorthand.

A

[Ar], (4S)2

77
Q

Write the electric configuration of zinc in shorthand.

A

[Ar], (4S)3, (3D)10

78
Q

What is the definition of the first ionisation energy?

A

The energy required to convert 1 mole of gaseous atoms into 1 mole of +1 cations, each atom losing 1 electron.

79
Q

What is the general formula for the first ionisation energy?

A

M(g) (arrow) M(g)+ + e-

Where M= a metal.

80
Q

What is the rule of ionisation energies when the element has 3d and 4S orbitals with electrons in it?

A

The 4S electrons are lost first.

81
Q

When the ionisation energies of an element are small the electrons are said to be…?

A

In the same shell.

82
Q

When the ionisation energies of an element have large jumps the electrons are said to be…?

A

In different shells.

83
Q

What are the reasons for smaller ionisation energies?

A

The shielding effect - more electrons in the atom mean that the outer electron is more repelled. The nuclear charge is getting bigger but because there are more full shells of electrons between nucleus and the outer electron, there’s an increased shielding effect resulting in a lower ionisation energy.

84
Q

What is the trend in ionisation energies across the period?

A

The general trend is an increase in ionisation energy due to an increase of nuclear charge

85
Q

What are the reasons for the trend in the periods?

A

The nuclear charge is increasing due to the electron going into the same shell. There’s no increase in shielding and the atomic radii decreases. There’s a greater attraction of the outer electron meaning that the ionisation energy increases.

86
Q

Why does boron have a lower ionisation energy than beryllium?

A

Because there’s a greater shielding effect in the 2S electrons in boron.

87
Q

Why does oxygen have a lower ionisation energy than nitrogen?

A

Because oxygen has an electron pair which causes more repulsion compared to nitrogen which has no electron pairs.

88
Q

State the number of protons in a Ca+2 ion.

A

20

89
Q

Write an equation that represents the first ionisation energy of potassium.

A

K(g) (arrow) k(g)+ + e-

CH 1 (8 decks)

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