Brainscape's Knowledge GenomeTM

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


See full index

Chemistry IGCSE > Ions & Bonding > Flashcards

Ions & Bonding Flashcards

1
Q

define atom

A

the smallest unit of matter that retains its properties

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

what are the 3 subatomic particles?

A

protons, neutrons and electrons

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

how is the mass number calculated?

A

number of protons + number of neutrons

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

how is the number of neutrons calculated?

A

mass number - atomic number

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

how is the atomic number calculated?

A

number of protons

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

define isotopes

A

variations of the same element with different numbers of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what subatomic particle affects the chemical properties of an element?

A

electrons

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

do the physical properties change depending on the different isotopes of an element?

A

yes

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

what physical properties vary between isotopes?

A

masses
densities
mpt / bpt

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

how is the average mass of an element calculated?

A

isotope 1 (abundance x mass/ 100) + isotope 2 (abundance x mass/100)

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

Define ion

A

charged atoms or molecules

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

which is positive and which is negative; cations and anions

A

cations are positive and anions are negative

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

Define bonding

A

the forces between particles that cause them to stick together

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

Define structure

A

the 3D arrangement of particles as a consequence of bonding

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

Define lattice

A

a repeating pattern of particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Define discrete

A

individual particles not arranged in a pattern

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

Define allotropes

A

different structural forms of the same element (same chem. properties, different physical properties)

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

Halogens exist as…

A

diatomic molecules held together by a single covalent bond

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

What are the predicted properties of halogens?

A
  1. low mpt (weak IMFs)
  2. do not conduct
  3. soluble only in oil-like substances
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the standard state color (aq) of:

F₂
Cl₂
Br₂
I₂

A

F₂ : (g) pale yellow (aq) colorless
Cl₂ : (g) pale green (aq) pale yellow
Br₂: (l) red/brown (aq) orange
I₂ : (s) grey (aq) brown/orange

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

What is the relationship of mpt from F₂ - At₂

A

mpt inscreases from F₂ to At₂ because the particles get bigger and there is a larger surface area (more IMFs)

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

Test 1 for halogens (damp blue litmus paper and starch)

A

Cl₂ damp blue litmus→red→white

Br₂ damp blue litmus→red→white
(slow)

I₂ starch→blue/black

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Test 2 for halogens (hexane test)

A

Cl₂ hexane→colorless

Br₂ hexane→orange

I₂ hexane→pink

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

Cl₂ + H₂O→
Br₂ + H₂O→

A

HCl + HOCl
HBr + HOBr

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

What color did the reaction of Fe and Cl₂ glow?

A

red

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

What happens to the mpt to alkaline earth metals (group 2)?

A

the mpt decreases but it is always higher than Group 1 due to the higher magnitude of charge and more delocalised electrons

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

What happens to the reactivity of Alkaline group metals (group 2)?

A

the reactivity increases but it is always lower than group 1 because they need to lose 2 electrons, not just 1

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

What are the 4 properties of transition metals?

A
  • high mpt (higher than group 1 & 2)
  • high density
  • variable charges (2+,3+, → 8+)
  • form colored compounds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are the colors of the following ions

Fe²⁺
Fe³⁺
Cu²⁺
Mn²⁺
Mn⁷⁺
Cr³⁺
Cr⁶⁺

A

Fe²⁺……………..green
Fe³⁺……………..orange/brown
Cu²⁺……………..blue
Mn²⁺…………….pink
Mn⁷⁺…………….purple
Cr³⁺………………green
Cr⁶⁺………………bright orange

30
Q

Define inert

A

a full outer energy level which causes the atom to be unreactive

31
Q

What are the properties of noble gases?

A
  • very low mpt (weak inter-atomic forces)
  • do not conduct
  • insoluble in water
  • no bonding, exist as single atoms
  • full outer energy level
32
Q

What are some of the uses for the following elements?

He
Ne
Ar

A

He………….balloons / air-ships (less dense than air)
Ne………….lighting (produces color with electricity)
Ar…………..light-bulbs (inert atmosphere)

33
Q

What is electronic configuration?

A

(x,y,z)

34
Q

How many energy levels do atoms have?

A

7

35
Q

Why does the process of loss of electron require little energy?

A

1) electrons are located on the outside of an atom

2) electrons have small masses

36
Q

How can the numbers of protons or neutrons be changed?

A

nuclear reactions

37
Q

Why do atoms tend to lose or gain electrons?

A

to fully occupy their outer energy level

38
Q

Where does ionic bonding occur?

A

in compounds containing a metal and a non-metal

39
Q

GO MEMORISE THE TABLE MALU SENT TO YOU

A

ok…

40
Q

Define ionic bond

A

electrostatic force of attraction between oppositely charged ions

41
Q

Why do ions attract in multiple directions?

A

because they are spheres (causes formation of a lattice)

42
Q

Describe structure of NaCl

A

lattice of alternating cations and anions held together by electrostatic forces

43
Q

Define properties

A

characteristics of chemicals

44
Q

What are some properties that substances can have?

A

1) mpt / bpt
2) electrical conductivity
3) solubility
4) malleability

45
Q

What does the strength of forces between particles depend on?

A

1) magnitude of charge
2) radius or ions (size)

46
Q

Define electrical conductivity

A

charged particles that can move without breaking forces

47
Q

In what states can ionic substances conduct?

A

liquid or aqueous

48
Q

What are the 4 properties of ionic substances?

A

1) high mpt
2) conduct as (l) or (aq)
3) dissolve in water
4) brittle

49
Q

What does malleability depend on?

A

forces present when particles move

50
Q

Where does covalent bonding occur?

A

in substances containing 2 or more non-metals

51
Q

How can covalent bonding be shown on a diagram?

A

bonding diagram or displayed formula

52
Q

Define covalent bond

A

the electrostatic attraction of 2 nuclei for a shared pair of electrons

53
Q

What are the 2 types of forces in a covalent discrete structure?

A

1) IMFs (weak)
2) covalent bonds (strong)

54
Q

What are the 3 properties of covalent discretes?

A

1) very low mpt
2) do not conduct
3) only soluble in oil-like substances

55
Q

Why do covalent discretes have a very low mpt?

A

because the IMFs are easy to break and mpt depends on the physical sie of the molecules

56
Q

Why do covalent discretes not conduct?

A

because there are no charged particles

57
Q

Why are covalent discretes only soluble in oil-like substances?

A

because during dissolving, molecules do not dissociate, the molecules only separate, meaning that only the IMFs need to be broken

58
Q

What are the 4 properties of SiO₂ (sand)?

A

1) very high mpt
2) doesn’t conduct
3) insoluble in all solvents
4) brittle

59
Q

Describe the structure of SiO₂

A

lattice of atoms held together by strong covalent bonds, not IMFs

60
Q

Pick the correct word to fill in the blanks:
words:【only one force/both forces】
Most covalent structures have ________________, covalent and/or discrete

A

only one force

61
Q

What are the 3 properties of diamond?

A

1) very high mpt (~3500 Cº)
2) does not conduct
3) does not dissolve in any solvent

62
Q

What are the only 3 covalent substances to have a lattice structure?

A

1) SiO₂
2) C in diamond
3) C in graphite

63
Q

What are the properties of graphite?

A

1) high mpt
2) conducts electricity due to delocalised electrons
3) insoluble in every solvent
4) lubricant, layers can slide over each other without affecting the rest of structure

64
Q

Where does metallic bonding occur?

A

metallic elements

65
Q

Describe a metallic element

A

a lattice of cations surrounded by delocalised electrons held together by strong electrostatic forces

66
Q

What are the 4 characteristics of metallic elements?

A

1) high mpt
2) conduct
3) insoluble in all solvents
4) malleable

67
Q

What is the relationship with color from F₂→At₂?

A

color becomes darker

68
Q

What is the relationship of alkali group 1 metals when moving down with mpt?

A

decreases

69
Q

What is the relationship of halogens group 2 non-metals when moving down with mpt?

A

increases

70
Q

What is the relationship of alkali group 1 metals when moving down with reactivity?

A

increases

71
Q

nvm

A
72
Q
A

Chemistry IGCSE (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions