Chemical Bonding

Question 1

3 types of bonding

Answer 1

Covalent , ionic , metallic

Question 2

How do atoms become stable/have full outer electron shells

Answer 2

1. Form ions (give away & accept electrons )
2. Form covalent bonds with another atom (share a pair of electrons )

Question 3

How is a covalent bond formed

Answer 3

A covalent bond forms when two non-metal atoms share a pair of electrons

held together by the electrostatic force of attraction between the positive nuclei of each atom and their negative electrons.

Question 4

What does a covalent bond and what does it occur with

Answer 4

A covalent bond is a Strong force of attraction occurs between non metal atoms

Question 5

How is a covalent discrete molecule form

Answer 5

(Most )Substance that form covalent bonds form individual or discrete molecules.

Question 6

How to tell that is is a covalent discrete molecule

Answer 6

You can count the number of atoms & write its chemical formula.
They have a low melting point/boiling point ( below 500C )

Question 7

What are covalent network structures

Answer 7

These are giant structures of nonmetal atoms held together by very strong covalent bonds , needing allot of energy to break them.

Question 8

How to tell it’s a covalent network structure

Answer 8

Impossible/very hard to count exact number of atoms
High melting/boiling point ( above 500C )

Question 9

Strong covalent bonds and weak intermolecular forces look like

Answer 9

Strong covalent bonds - black lines
Weak intermolecular forces - dashed lines

Question 10

What chemical formula is buckminsterfullerene

Answer 10

C60

Question 11

What are allotropes

Answer 11

Different forms of the same element

Question 12

What is the most well known allotrope

Answer 12

Carbon

Question 13

How does ionic bonding form

Answer 13

Forms between ions of metal & non metals

Question 14

What kind of attraction does ionic bonding have

Answer 14

Very strong force of attraction

Question 15

What is an ionic bond

Answer 15

Electrostatic attraction between oppositely charged ions

Question 16

What makes up an ionic lattice( held up by what)

Answer 16

Ionic compounds held in place by strong ionic bonds

Question 17

How to melt ionic bonds

Answer 17

Using allot of energy because of a high melting/boiling point

Question 18

(Solubility) what did covalent and ionic substances dissolve

Answer 18

Covalent substances tend to dissolve other covalent substances
Ionic substances tend to dissolve other ionic substances

Question 19

What does it mean to be soluble

Answer 19

The ability to be dissolved

Question 20

Why is water a polar molecule

Answer 20

Because the electrons between oxygen and hydrogen atoms in water are not shared equally

Question 21

What does is mean that water is a polar molecule

Answer 21

One side of the molecule is slightly positive
other side of the molecule is slightly negative

Question 22

What can the polar molecule dissolve

Answer 22

Despite being covalent , water can dissolve ionic compounds but not covalent compounds

Question 23

Do ionic compounds conduct or not

Answer 23

They do conduct electricity when they are in solution or melted to form a liquid as the ions can move

Question 24

Do covalent compounds conduct electricity or not

Answer 24

They do not conduct electricity in any state

Question 25

What is the only acceptation to covalent compounds trying to conduct

Answer 25

Covalent compounds don’t conduct whereas carbon in the form of graphite even though it’s a covalent compound it does conduct

Question 26

What is metallic bonding

Answer 26

electrostatic attraction between positively charged metal ions and a sea of delocalised (free) negative electrons

Question 27

What does it mean to be delocalised with metallic bonding

Answer 27

It means that they are free to move , allowing them to carry an electric charge through metallic structure

Question 28

What is electrolysis

Answer 28

It is the (break down ) of ionic compounds using electricity

Question 29

What ions are attached to what ( electrolysis)

Answer 29

Positive ions are attached to negative electrodes & negative ions are attached to positive electrodes

Question 30

What is an example of an electrolysis experiment

Answer 30

Copper chloride solution being broke down using electricity to form copper & chloride

Question 31

Where do covalent discrete molecules conduct electricity

Answer 31

They don’t conduct it in liquid , solid or solution

Question 32

Where do covalent network conduct electricity

Answer 32

They don’t conduct it in solution , solid or liquid

Question 33

Where do ionic bonds conduct electricity

Answer 33

Solid - they don’t conduct Liquid - they conduct Solution - they conduct

Question 34

Where do metallic bonds conduct electricity

Answer 34

Solid -they conduct Liquid - they conduct Solution- in soluble

Question 35

Most covalent substances don’t dissolve in water however what do they dissolve in

Answer 35

They do dissolve in oil.

Question 36

What is a molecule

Answer 36

A molecule is a group of atoms held together by covalent bonds.

Question 37

What is a diatomic molecule

Answer 37

Element Which is made of 2 atoms e.g H2 or N2

Question 38

What are balloon/petal diagrams used to show

Answer 38

how the outer electrons are shared between atoms to form covalent bonds.

Question 39

Examples of covalent network

Answer 39

diamond (carbon), sand (silicon dioxide) and graphite (carbon).

Question 40

How to break an ionic lattice

Answer 40

Ionic compounds dissolve in water. When they dissolve in water the lattice breaks up. Solutions of ionic compounds can be broken down using a process called electrolysis

Question 41

What is the only Liquid Metal ( metallic bonding)

Answer 41

Most metals are solids. Mercury is the only liquid metal.

Question 42

Why can metals conduct electricity

Answer 42

As electrons can move from metal ion to metal ion, metals conduct electricity.

Question 43

What is a covalent discrete molecule

Answer 43

A covalent molecule in which the Intermolecular forces are really weak