Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

N4 chemistry > Atomic Bonding + Structure > Flashcards

Atomic Bonding + Structure Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are atoms like in a compound?

A

Two or more different types of atoms are joined together.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Where does the name of compounds come from?

A

The names of the elements in them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What do chemical compound formulae contain?

A

Element symbols and numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What do prefixes tell you in compound names?

A

How many atoms of an element there are in a compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is an atom?

A

Smallest particle of a chemical element that still has its properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is all matter composed of?

A

Atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What do chemical reactions do?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How are all elements organised?

A

Into a grid structure known as the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are the columns in the periodic table called?

A

Groups

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the rows in the periodic table called?

A

Periods

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What do metalloids have?

A

Properties that are similar to both metals and non-metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What will decreasing temperature do to gases and liquids?

A

Make gases turn into liquids and liquids turning into solids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

At what temperature will all elements exist as solids?

A

-237.15°c (absolute 0)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What will increasing temperature do?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

At what temperature will all elements exist as gases?

A

5590°C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How many named groups are there in the periodic table?

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What do elements in the same group have?

A

Similar chemistry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

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

A

7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

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

A

Diatomic elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Why do we call them diatomic?

A

They exist in molecules of two atoms each

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Name the 7 diatomic elements

A

Hydrogen
Oxygen
Nitrogen
Fluorine
Chlorine
Bromine
Iodine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are atoms made up of?

A

Subatomic particles
Protons, neutrons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

How can each atom be described?

A

Two numbers, the atomic number and the mass number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is the atomic number?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the mass number?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

How can we calculate the number of neutrons?

A

No. of neutrons = mass number - atomic number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

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

A

Larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What does nuclide notation show?

A

The contents of the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

How are electrons arranged?

A

Around the nucleus in discrete (separate) shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What can each shell fit?

A

A specific number of e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions