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N4 chemistry > Atomic Bonding + Structure > Flashcards

Atomic Bonding + Structure Flashcards

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1
Q

What are atoms like in an element?

A

All the atoms are the same type.
It can’t be broken down into simpler substances

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2
Q

What are atoms like in a compound?

A

Two or more different types of atoms are joined together.

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3
Q

Where does the name of compounds come from?

A

The names of the elements in them

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4
Q

How do we name compounds with two elements?

A

The name of the first element stays the same, the ending of the second element changes to ide

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5
Q

How do we name compounds with three elements and one is oxygen?

A

Name of first element stays the same.
Name of the second element can be shortened.
Last part of the name changes to ate

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6
Q

What do chemical compound formulae contain?

A

Element symbols and numbers

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7
Q

What do the numbers represent in chemical compound formulae?

A

How many types of atom there are.
If there is no number next to an element symbol, that means there is only one type of that atom

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8
Q

What do prefixes tell you in compound names?

A

How many atoms of an element there are in a compound

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9
Q

What are the prefixes for 1,2,3,4 no. of atoms?

A

1- Mono
2- Di
3- Tri
4- Tetra

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10
Q

What is an atom?

A

Smallest particle of a chemical element that still has its properties

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11
Q

What is all matter composed of?

A

Atoms

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12
Q

What do chemical reactions do?

A

Join or split atoms to rearrange them, but they can’t change one element into another

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13
Q

How are all elements organised?

A

Into a grid structure known as the periodic table

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14
Q

What are the columns in the periodic table called?

A

Groups

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15
Q

What are the rows in the periodic table called?

A

Periods

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16
Q

Is there a clear boundary between metals and non-metals?

A

No, instead there is a number of ‘in-between’ elements called semi metals/metalliods

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17
Q

What do metalloids have?

A

Properties that are similar to both metals and non-metals

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18
Q

What will decreasing temperature do to gases and liquids?

A

Make gases turn into liquids and liquids turning into solids

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19
Q

At what temperature will all elements exist as solids?

A

-237.15°c (absolute 0)

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20
Q

What will increasing temperature do?

A

Have a reverse effect. Solids turn into liquids and liquids turn into gases

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21
Q

At what temperature will all elements exist as gases?

A

5590°C

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22
Q

How many named groups are there in the periodic table?

A

3

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23
Q

Name the named groups in the periodic table and their groups

A

Group 1- Alkali metals
Group 7- Halogens
Group 8/0- Noble gases

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24
Q

What do elements in the same group have?

A

Similar chemistry

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25
Q

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

A

7

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26
Q

What do we call elements that don’t exist as a single atom?

A

Diatomic elements

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27
Q

Why do we call them diatomic?

A

They exist in molecules of two atoms each

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28
Q

Name the 7 diatomic elements

A

Hydrogen
Oxygen
Nitrogen
Fluorine
Chlorine
Bromine
Iodine

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29
Q

What are atoms made up of?

A

Subatomic particles
Protons, neutrons and electrons

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30
Q

How can each atom be described?

A

Two numbers, the atomic number and the mass number

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31
Q

What is the atomic number?

A

No. of protons. No two elements have the same atomic number

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32
Q

What is the mass number?

A

No. of protons + neutrons (all particles that have a mass)

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33
Q

How does the atomic number always increase?

A

By one as you go across a period in the periodic table.
You can’t skip a number

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34
Q

How can we calculate the number of neutrons?

A

No. of neutrons = mass number - atomic number

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35
Q

What is mass number always compared to atomic number (except for H)

A

Larger

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36
Q

What do atoms charge =?

A

Atoms are neutral so charge = 0, so the number of p+ and e- must be the same.
This means that the no. of e- must be the same as the atomic number

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37
Q

What does nuclide notation show?

A

The contents of the nucleus

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38
Q

How do we write the mass & atomic numbers when writing the nuclide notation?

A

They must always be written to the left of the element symbol

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39
Q

How are electrons arranged?

A

Around the nucleus in discrete (separate) shells

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40
Q

What can each shell fit?

A

A specific number of e-

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41
Q

What is the outermost shell containing e- called?

A

Valence shell

42
Q

What are the e- in the valence shell called?

A

Valence e-

43
Q

Why is the smallest shell first when arranging electrons?

A

It’s closest to the positive nucleus

44
Q

Can you skip a shell?

A

No

45
Q

What do negative e- do?

A

Repel one another (same charge) and will try to get as far away from each other as possible
(4 sides of nucleus, single e-)

46
Q

What happens where there are no more ‘single seats’ left?

A

e- will pair up

47
Q

What are noble gases the only element to have?

A

Full outer shells
The group no. is the same as the no. of valence e-
The period no. is the same as the no. of occupied e- shells

48
Q

What is an ion?

A

A charged atom

49
Q

How are ions formed?

A

When atoms gain or lose e-

50
Q

How are ions charged?

A

The no. or p+ and e- is not equal

51
Q

What do atoms have to do to gain a full outer shell?

A

Gain or lose e-, this makes them more stable

52
Q

What do ions have the same electron arrangement as?

A

The nearest noble gas

53
Q

What do metals atoms lose and form?

A

e- and they form + ions

54
Q

What do non-metal atoms gain and form?

A

Gain e- and form - ions

55
Q

What do negative ion names end in?

A

-ide

56
Q

Why do metals lose e-?

A

Their valence shells are less than half full, so it takes less energy to lose e- than gain them.

The opposite is true for non-metals

57
Q

How are ionic charges written?

A

A number followed by + or -.
Eg, a 2 positive charge is written as 2+

58
Q

How can we calculate ionic charge?

A

No. of P+ - no. of e-

59
Q

What does gaining e- do?

A

Forms negative ions (more negative charges)

60
Q

What does losing e- do?

A

Forms positive ions (more positive charges)

61
Q

What does the formula of a compound depend on?

A

The valency of each element involved.

62
Q

What is valency?

A

The no. of bonds an atom can make.
This is related to the no. of valence e-

63
Q

What is the valency for group 1-4?

A

It’s the same as the no. of valence e-

64
Q

What is the valency for group 5-7?

A

It’s the same as the no. of e- needed to gain a full outer shell

65
Q

What is the valency for group 8/0?

A

They’re noble gases, which don’t form bonds because they already have full outer shells.
Valency = 0

66
Q

What do some elements have?

A

Multiple possible valencies

67
Q

How should transition metals have their valency shown?

A

A Roman numeral

68
Q

How can we use valency?

A

To work out how many of each type of atom are bonded in a compound

69
Q

What should happen to ‘arms’ in a compound?

A

In a compound all ‘arms’ must be paired up

70
Q

What is the formula mass of a compound?

A

The sum of all the masses of all the atoms present

71
Q

How do we calculate the formula mass or a compound?

A
  1. Write the formula of the compound
  2. Find the mass of each element and multiply by the no. of atoms present
  3. Add up all the masses
72
Q

How can the atoms in a compound be joined up?

A

A) Ionic bonds firm between metals and non-metals, eg. NaCl

B) Covalent bonds form between non-metal atoms, eg. CO2

73
Q

What will the type of bonding in a compound affect?

A

It’s physical properties, such as boiling and melting point, hardness and conductivity

74
Q

What do different bonds equal?

A

Different bonds = different properties

75
Q

What is an ionic bond?

A

The electrostatic force of attraction between ions with opposite charges ( + and -)

76
Q

How is ionic bonds formed?

A

When valence e- are completely transferred from a metal atom to a non metal atom

77
Q

What can non-metals share e- with?

A

Other non-metal atoms to gain a full outer shell

78
Q

What is a covalent bond?

A

The attraction between two positive nuclei have for a shared pair of e-

79
Q

How can we use dot and cross diagrams?

A

To show how e- are arranged in molecules

80
Q

What do dot and cross diagrams only show and why?

A

The valence e- because they are involved in bonding

81
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 middle

82
Q

Why are atoms overlapped?

A

To give each atom a share of enough e- to give them a full outer shell (usually 8 e-, 2 for H)

83
Q

How do we draw a dot and cross diagram?

A

1) Draw the atoms with only their valence e-, eg for water (H2O)

2) Put the atoms together and check if they have a full outer shell (2 for H, 8 for O)

84
Q

What do the physical properties of a chemical substance depend on?

A

The type of bonding present (ionic or covalent)

85
Q

Name the following properties affected

A

Melting point (temp at which substance switches between a solid/liquid)

Boiling point (temp at which a substance switches between a liquid/gas)

State at a room temp (solid, liquid or gas)

Conductivity (can it conduct electricity?)

86
Q

What do covalent bonds usually consist of?

A

Discrete (separate) molecules

87
Q

What are covalent substances?

A

Elements and compounds made up or non-metals (eg Cl2, H2O)

88
Q

What are the attractions between molecules like?

A

Weak and require little energy (low temp) to break

89
Q

What do covalent substances have?

A

Low melting and boiling points. They can be solid, liquid or gas at room temp.

90
Q

What do covalent substances not do?

A

Conduct electricity in any state

91
Q

What are ionic substances usually?

A

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

92
Q

What do ionic compounds not form?

A

Molecules. They form huge lattice structures

93
Q

What is a lattice?

A

Grid-like arrangement.

94
Q

How is a lattice held together?

A

By a strong electrostatic attractions between + and - ions. These attractions are ionic bands

95
Q

Why do ionic compounds have high melting and boiling points?

A

Ions are held together by strong ionic bonds.

96
Q

What do ionic substances require to break?

A

A lot of energy (high temp) is required to break them

97
Q

When are ionic substances solids?

A

At room temp (25 °C)

98
Q

How can a substance conduct electricity?

A

It must have a flow of charged particles

99
Q

Why can’t ionic solids move freely?

A

Charged particles (ions) can’t move freely because they are locked in a lattice

100
Q

What happens if an ionic solid is molten or dissolved in water?

A

It will be able to conduct because the ions will be able to move freely

N4 chemistry (3 decks)

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