Topic 2 Structure and bonding Flashcards

1
Q
  1. What can link two atoms together?
A

a bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q
  1. Which group of elements is stable and doesnt form compounds easily?
A

noble gases/group 0 in the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q
  1. How is an elements electron arrangement linked to its position in the periodic table?
A

Elements in the same group have the same number of electrons in their outer shell.

Elements in the same period have the same amount of electron shells.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q
  1. How do positive and negative charges affect each other?
A

They attract each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q
  1. Which sub-atomic particles of atoms take part in chemical reactions?
A

electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q
  1. What is an ion?
A

an atom that is charged because it has lost or gained one or more electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q
  1. What happens when an ionic bond is formed?
A

One atom loses electrons to another atom to form oppositely charged ions that attract each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q
  1. Which kinds of elements are usually involved in the formation of ionic bonds?
A

metals and non-metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q
  1. How is a positive ion formed and what is it called?
A

formed by the loss of electrons; cation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q
  1. How is a negative ion formed and what is it called?
A

formed by the gain of electrons; anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q
  1. What are the forces called that hold ions together?
A

electrostatic forces / electrostatic attractions / ionic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q
  1. Why do atoms form ions?
A

to become more stable (like a noble gas)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q
  1. Explain why group 1 elements such as sodium and lithium form a 1+ ion.
A

They both have one electron in their outer shell and lose it to become stable.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q
  1. What are the charges on calcium, oxide and chloride ions?
A

2+, 2- and 1-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q
  1. What structure of regularly repeating ions do ionic compounds form?
A

lattice structure / ionic lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q
  1. What is the formula of the nitrate ion?
A

NO3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q
  1. What is the general name for a positive ion?
A

cation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q
  1. What is the general name for a negative ion?
A

anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q
  1. What is the charge on the ions of elements in group 1 of the periodic table?
A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q
  1. What is the charge on the ions of elements in group 6 of the periodic table?
A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q
  1. What happens to the electrons in the outer shell of metal atoms when they form ions?
A

they are lost

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q
  1. What is the name of the ionic compound containing calcium and bromine only?
A

calcium bromide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q
  1. What is the name of the ionic compound containing potassium, chlorine and oxygen?
A

potassium chlorate (any element combined with oxygen is an ___ate )

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q
  1. What does a bond do in an element or compound?
A

holds atoms together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q
  1. What are electrostatic forces of attraction?
A

attractions between positive and negative charges (positive and negative ions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q
  1. Which part of an atoms structure is most involved when two atoms react?
A

the electrons (because they are on the outside of atoms)

27
Q
  1. How many electrons are in the outer shell of the elements in groups 5, 6 and 7?
A

5, 6 and 7

28
Q
  1. What kind of electron arrangement is most stable?
A

a complete/full outer shell

29
Q
  1. What is the molecular formula of the very common compound formed between hydrogen and oxygen?
A

H2O

30
Q
  1. How many more electrons does an oxygen atom need to get a complete outer shell?
A

2 more (it gains two electrons and becomes a 2- ion)

31
Q
  1. What are molecules?
A

groups of atoms held together by (covalent) bonds

32
Q
  1. Which type of atoms are covalent bonds found between
A

non-metal and non-metal

33
Q
  1. What is a covalent bond?
A

a shared pair of electrons

34
Q
  1. What happens to electrons between two atoms in a covalent bond
A

they are shared

35
Q
  1. What kinds of elements usually form molecules?
A

non-metals

36
Q
    1. What kinds of bonds are found in molecules?
    1. What kinds of bonds are found between molecules?
A

covalent bonds are found holding the atoms together in molecules.

intermolecular forces are found between molecules.

37
Q
  1. What is the name of the type of bond formed by sharing electron pairs within molecules?
A

covalent bond

38
Q
  1. What term describes the number of atoms of each element bonded together in a molecule?
A

molecular formula (e.g. the molecular formula of a molecule of water is H2O)

39
Q
  1. In oxygen and carbon dioxide, the atoms share two pairs of electrons. How do we describe these bonds?
A

double bonds (represented by = in a displayed formula)

40
Q
  1. What is the name of the force that holds molecules together in gases and liquids
A

intermolecular force

41
Q
  1. How strong are the forces of attraction between molecules compared to the bonds within molecules?
A

They are relatively weak. (Covalent bonds holding atoms together are strong / Intermolecular forces holding molecules together are weak)

42
Q
  1. Are simple molecules usually good conductors of electricity at room temperature?
A

No, they are poor conductors of electricity (as they have no charged particles)

43
Q
  1. In what types of bonds are pairs of electrons shared?
A

covalent bonds

44
Q
  1. What are intermolecular forces?
A

forces of attraction between molecules

45
Q
  1. Do simple molecules have strong intermolecular forces between them?
A

No. They are described as weak.

46
Q
  1. Why are simple molecules poor conductors of electricity?
A

There are no charge carriers.

47
Q
  1. What can you say about the formula of small, simple molecules?
A

They are fixed.

48
Q
  1. What type of bonding is between the atoms in a molecule of water?
A

covalent

49
Q
  1. What type of structure does water have?
A

simple molecular / simple covalent

50
Q
  1. What strength of forces are there between different molecules of water?
A

weak (weak intermolecular forces)

51
Q
  1. Does pure water conduct electricity?
A

no (Most water contains dissolved ions which makes it conduct. Pure water has no charge carriers)

52
Q
  1. What type of structure do diamond and graphite have?
A

giant covalent, giant molecular

53
Q
  1. What does the term malleable mean?
A

can be hammered or bent into a different shape

54
Q
  1. What type of bonding does copper have?
A

metallic

55
Q
  1. What atoms does metallic bonding happen between?
A

metal and metal (i.e it is found in metals!)

56
Q
  1. What holds ions of metals together in a metallic bond?
A

a sea of delocalised electrons

57
Q
  1. Why can metals conduct electricity?
A

electrons are free to move and carry charge

58
Q
  1. What is a metallic bond?
A

the attraction between positive ions and delocalised electrons

59
Q
  1. What are the particles inside a metal?
A

metal ions surrounded by sea of electrons

60
Q
  1. Metals are ductile. What does ductile mean?
A

It can be drawn for example into wires

61
Q
  1. What can graphite by used as a conductor of electricity?
A

An electrode in electrolysis.

62
Q
  1. What happens to the particles during melting?
A

During melting the particles gain energy and more about move so they can move over each other

63
Q
  1. How is nitrogen and oxygen obtained from the air?
A

Fractional distillation of their liquid forms, cool air down first.

64
Q
  1. Why does oxygen have a low boiling point?
A

There are weak forces of attraction between the oxygen molecules.