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N5 Chemistry > Atomic bonding and structure > Flashcards

Atomic bonding and structure Flashcards

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1
Q

How are all elements organised?

A

Into a grid structure called the period table

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2
Q

What are the columns in the periodic table called?

A

Groups

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3
Q

What are the rows in the period table called?

A

Periods

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4
Q

What do elements in the same group have?

A

Similar chemical properties (they react similarly with certain chemical substances)

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5
Q

What are the three names groups?

A

Group 1- alkali metals
Group 7- halogens
Group 8 (or 0)- noble gases

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6
Q

How many elements in the periodic table don’t exist as single atoms?

A

7

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7
Q

What are elements called when they don’t exist as single atoms?

A

Diatomic

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8
Q

Why are elements called diatomic?

A

They exist in molecules of two atoms each

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9
Q

Name the seven diatomic elements

A

H2, N2, O2, F2, Cl2, Br2, I2

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10
Q

What are atoms made up of?

A

3 types of subatomic particles
Protons
Neutrons
Electrons

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11
Q

What charge do protons have?

A

Positive

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12
Q

What charge do neutrons have?

A

Neutral (0)

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13
Q

What charge do electrons have?

A

Negative charge

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14
Q

Where are protons located in an atom?

A

Nucleus

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15
Q

Where are neutrons located in an atom?

A

Nucleus

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16
Q

Where are electrons located in an atom?

A

Electron shells

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17
Q

How can each atom be described?

A

Two numbers
No. of protons and mass number

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18
Q

What is the number of protons also known as?

A

Atomic number and it’s unique to every single element

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19
Q

What is the mass number?

A

No. of protons + neutrons

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20
Q

Why are atoms neutral?

A

Number of protons is the same as number of electrons

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21
Q

What does energy levels mean?

A

Electrons are arranged around the nucleus in discrete (separate) shells

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22
Q

What is the outermost shell containing e- called?

A

Valence shell

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23
Q

What is the e- called that resides in the valence shell?

A

Valence e-/ outer e-

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24
Q

Why is the smallest shell filled in first?

A

Closest to the positive nucleus (which e- are attracted to)

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25
Q

What are noble gases the only element to have?

A

Full outer shells

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26
Q

What is the group number the same as?

A

No. of valence e-

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27
Q

What is the period number the same as?

A

The no. of occupied e- shells

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28
Q

What is an ion?

A

Charged atom

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29
Q

When is an ion formed?

A

When an atom loses or gains e-

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30
Q

Why do atoms lose or gain e-?

A

To get a full outer shell. This makes the more stable

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31
Q

What do ions have the same electron arrangement as?

A

The nearest noble gas

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32
Q

What do non-metal atoms gain and form?

A

Gain e-, form negative ions

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33
Q

What do metal atoms lose and form?

A

Lose e- and form positive ions

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34
Q

What are isotopes?

A

Atoms of the same atomic number (same element) with different mass numbers.

No. of p+ is the same, but no. of n° is different

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35
Q

What can use nuclide notation to do?

A

Distinguish between different isotopes

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36
Q

What is carbon dating?

A

Using carbon-14 atoms to find out the age of long-dead organisms.

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37
Q

What is carbon-14 and what does it mean?

A

Radioactive.
This means that when a living organism dies, the carbon-14 atoms it contains gradually decays into more stable carbon atoms

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38
Q

What are not all isotopes?

A

Equally abundant.
Generally, stable isotopes are abundant, while unstable isotopes are found only in trace amounts

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39
Q

What does isotopes stability depend on and why does this happen?

A

The number of neutrons in the nucleus. Too many or too few will make it unstable.

This happens because neutrons play an important role in minimising repulsions between positively charged protons. Since neutrons themselves have no charge, they act as a ‘buffer’ between protons. play an important role in

40
Q

How many isotopes does copper have?

A

Two 63Cu and 65Cu

41
Q

What is relative atomic mass?

A

Average mass of all isotopes of an element taking into account their relative abundance

42
Q

When can RAM be calculated?

A

If the abundance of each isotope of an element is known

43
Q

What are noble gases?

A

Monatomic

44
Q

What does monatomic mean?

A

They exist as single atoms

45
Q

Why are noble gases monatomic?

A

They already have full outer shells which makes them very stable

46
Q

How can other elements obtain stable e- configuration?

A

The can form ions by losing or gaining electrons, or form covalent bonds to achieve full outer shells and become more stable

47
Q

When does a covalent bond form?

A

When two positive nuclei are held together by their common attraction for a shared pair of electrons.

48
Q

Where do covalent bonds usually form?

A

Between non-metal atoms

49
Q

What can we use a dot and cross diagram for?

A

Show how e- are arranged in molecules

50
Q

What do dot and cross diagrams only show?

A

How the valence e- because they are only ones involved in bonding

51
Q

Why are atoms overlapped in dot and cross diagrams?

A

To give each atom a share of enough e- to give them a full outer shell

52
Q

How are e- drawn in dot and cross diagrams?

A

Dots for one atom and crosses for the other with shared pairs of e- drawn in the overlap area

53
Q

What are structural formulae used to show?

A

The number of bonds between atoms in a molecule

54
Q

What do each bond between two atoms represent?

A

One pair of e- being shared

55
Q

What can covalent molecules adopt?

A

A number or common shapes

56
Q

What can we often do when predicting a shape of a compound?

A

Often we can predict a shape of a compound by counting the no. of atoms in the molecule

57
Q

What do simple lines represent when drawing 3D shapes on paper?

A

These bonds are on the same plane as the paper

58
Q

What do dashed lines represent when drawing 3D shapes on paper?

A

These bonds are behind the paper

59
Q

What do wedges represent when drawing 3D shapes on paper?

A

These bonds are in front of the paper (pointing towards you)

60
Q

What will all two atom molecules be and most molecules containing double/triple bonds

A

Linear

61
Q

What often are 3 atom molecules containing only single bonds?

A

Angular

62
Q

What is the reason for angular shapes?

A

Is usually e- pairs nor engaged in bonding repelling shared e- pairs, changing the shape of the molecule

63
Q

What shape do 4 atom molecules adopt?

A

Trigonal pyramidal

64
Q

What is the most common trigonal pyramidal?

A

Ammonia

65
Q

What shape do molecules containing boron adopt?

A

Trigonal planar shape

66
Q

What shape do molecules containing 5 atoms often adopt?

A

Tetrahedral structure

67
Q

In covalent substances how are atoms held together?

A

Covalent bonds

68
Q

What are the two types of covalent structures?

A

Molecular
Network

69
Q

Do covalent substances conduct electricity?

A

No except for graphite

70
Q

What are covalent molecular elements and compounds made up of?

A

Discrete molecules

71
Q

What does each discrete molecule contain?

A

Few atoms bonded together

72
Q

Do covalent molecular elements have strong or weak forces of attraction between molecules?

A

Weak. They are broken when a substance boils (covalent bonds are not broken)

73
Q

What are the properties of covalent molecular structure?

A

Low melting and boiling points due to weak attractions between molecules

Can be gas, liquid or solid at room temp

Some can dissolve in water

74
Q

What temperature is room temperature?

A

25°C

75
Q

What happens to molecular substances that don’t dissolve in water?

A

They will usually dissolve in other solvents, e.g hexane

76
Q

What are covalent network elements and compounds made up of?

A

Thousands of atoms bonded together

77
Q

What are the only network elements?

A

Boron, silicon and carbon

78
Q

Silicon carbide and silicon dioxide are what?

A

Network compounds

79
Q

What is the major component in sand and glass?

A

Silicon dioxide (SiO2)

80
Q

What is the formula for all covalent network compounds?

A

Ratio of different atoms in the giant structure

81
Q

What are the two common network forms of carbon?

A

Diamond and graphite

82
Q

What structure does diamond have compared to graphite?

A

A more regular structure with only strong covalent bonds throughout

83
Q

What are the properties of covalent network structures?

A

High melting + boiling points due to strong covalent bonds between all atoms

Solid at room temp

Doesn’t dissolve in any solvent

Hard, durable and extremely unreactive

84
Q

What are ionic substances usually?

A

Compounds made of metals and non-metals (eg. NaCl)

85
Q

What do ionic compounds form instead of molecules?

A

Huge lattice structures

86
Q

What is an ionic lattice?

A

A grid-like arrangement held together by strong electrostatic attraction between + and - ions

87
Q

Why do ionic compounds have high melting + boiling points?

A

They are held together by strong ionic bonds

88
Q

What is required to break ionic bonds?

A

A lot of energy (high temp)

89
Q

What are ionic substances at room temp?

A

Solids

90
Q

What are ionic compounds often in water?

A

Soluble

91
Q

What must a substance require to conduct electricity?

A

Flow of charged particles

92
Q

Why can’t ions move freely in ionic solids?

A

They are locked in a lattice

93
Q

What happens if an ionic solid is molten or dissolved?

A

It will be able to conduct as ions will be able to move freely

94
Q

What is the best way to determine the type of bonding between metallic, covalent network and ionic substances?

A

Conductivity test

95
Q

What state do metals conduct?

A

Solid and liquid

96
Q

What state do ionic compounds conduct?

A

Molten or dissolved

97
Q

What state do covalent networks conduct?

A

They don’t at all except graphite

N5 Chemistry (2 decks)

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