Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Grade 8 Science > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

In ionic bonding, what happens to the electrons

A

The electrons are transferred

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

In covalent bonding, what happens to the electrons

A

The electrons are shared

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

In ionic bonding, what is it between

A

Metal and non-metal

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

In covalent bonding, what is it between

A

Non-metals

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

In ionic bonding, what force holds it together (2)

A

Electrostatic force of attraction between oppositely charged ions (positive and negative)

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

Definition of compound (2)

A

DIFFERENT elements JOINED together

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

In covalent bonding, what happens to the electrons

A

The electrons are shared

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

In ionic bonding, what happens to the electrons

A

The electrons are transferred

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

In ionic bonding, what happens to the metal

A

Metal loses electrons to form a positive ion

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

In ionic bonding, what happens to the non-metal

A

Non-metals gain electrons to form negative ions

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

Ionic - description of melting point, and explanation (1+2)

A

High melting point
Strong electrostatic force of attraction that requires a lot of energy to break

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

Ionic - description of conductivity, and explanation (1+1)

A

Only conducts when molten or aqueous
The ions (charges) are free to move

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

Define molten

A

melted

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

Define aqueous

A

dissolved in solution

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

Simple covalent structure

A

Small molecule

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

How is simple covalent held together (2 - between atoms, between molecules)

A

Strong covalent bonds between atoms
Weak intermolecular forces between molecules

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

Simple covalent - description of melting point, and explanation (1+2)

A

Low melting point
It doesn’t require much energy to break the weak intermolecular forces

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

Simple covalent - description of conductivity, and explanation (1+1)

A

Does not conduct
There are no charged particles

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

Giant covalent structure

A

Giant lattice

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

How is giant covalent held together

A

Lots of strong covalent bonds

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

Giant covalent - description of melting point, and explanation (1+2)

A

High melting point
Requires a lot of energy to break the covalent bonds

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

Giant covalent - description of conductivity, and explanation (1+2)

A

Does not conduct except graphite
No free electrons except in graphite

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

Metallic structure (2)

A

Positive metal ions in a ‘sea’ of delocalised electrons

24
Q

Hot metallic is held together

A

Electrostatic force of attraction

25
Metallic - description of melting point, and explanation (1+2)
High melting point Strong electrostatic force of attraction that requires a lot of energy to break
26
Metallic - description of conductivity (1+1)
Yes, they conduct The electrons (charges) can move
27
atomic number
the number of protons and electrons in an atom
28
Lithium reaction with water: description, word equation, symbol equation
When lithium reacts with water, it sizzles and forms an alkaline solution - Lithium hydroxide Lithium + water > Lithium hydroxide + hydrogen 2Li + H2O > H2 + 2LiOH
29
Sodium reaction with water: description, word equation, symbol equation
When sodium reacts with water, it reacts more vigorously than lithium and forms an alkaline solution - Sodium hydroxide Sodium + water > Sodium hydroxide + hydrogen 2Na + H2O > H2 + 2NaOH
30
How do you calculate mass number
protons+neutrons
31
mass and charge of electron
Mass = 1/2000 Charge = negative
32
Mass and charge of neutron
Mass = 1 Charge = neutral
33
Mass number
The number of protons and neutrons combined
34
Mass and charge of proton
mass = 1 charge = +
35
maximum electrons in the 1st shell
2
36
maximum electrons in the 2nd shell
8
37
maximum electrons in the 3rd shell
8
38
Potassium reaction with water: description, word equation, symbol equation
When potassium reacts with water, it reacts more vigorously than sodium, burns with a lilac flame, produces a small popping noise, and forms an alkaline solution - Potassium hydroxide Potassium + water > Potassium hydroxide + hydrogen 2K + H2O > H2 + 2KOH
39
Trend in reactivity in group 1
Reactivity gets more vigorous as you go down the group
40
Trends in boiling/melting points in group 0 (noble gases)
They increase
41
Trends in boiling/melting points in group 1 (alkali metals)
They decrease
42
Trends in boiling/melting points in group 7 (halogens)
They increase
43
Sodium chloride what type of bond
ionic bond
44
Sodium chloride structure
giant ionic lattice
45
What holds sodium chloride together
electrostatic force of attraction holds the ions together
46
Explain why iodine has a low melting point(2)
Weak intermolecular forces that do not require a lot of energy to break Is a simple covalent (not giant covalent)
47
Explain, in terms of particles, why liquid iodine does not conduct electricity (2)
There are no free electrons so cannot carry charge through the structure
48
Describe and explain giant ionic melting point (3)
high melting point because strong electrostatic force of attraction that holds the ions together that requires a lot of energy to break
49
Describe and explain simple covalent melting point (3)
low melting point because weak intermolecular forces of attraction between molecules that do not require a lot of energy to break
50
Describe and explain giant metallic melting point (3)
high melting point because strong electrostatic force of attraction that holds the ions together that requires a lot of energy to break
51
Describe and explain giant covalent melting point (3)
high melting point because strong covalent bonds between non-metals that require a lot of energy to break
52
Describe and explain if giant ionic conducts (3)
only conducts when molten or aqueous because the ions (charges) are free to move
53
Describe and explain if simple covalent conducts (3)
Does not conduct because there are no charged particles
54
Describe and explain if giant metallic conducts (3)
Does conduct because the delocalised electrons (charges) can move
55
Describe and explain if giant covalent conducts (3)
Does not conduct EXCEPT for graphite because there are no free electrons except for in graphite, there are

Grade 8 Science (7 decks)

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