Ionic, covalent bonding

Question 1

What type of atoms usually participate in ionic bonding

Answer 1

atoms of non metal and metal

Question 2

what is the main characteristic of ionic bonding

Answer 2

a full outer shell

Question 3

what is a giant ionic lactice

Answer 3

a repeating structure formed by ionic bonds consisting (P+N) ions

Question 4

why do ionic compounds require a lot of energy to break their bond

Answer 4

because of the strong electrostatic attraction between ions

Question 5

why do noble gases have a strong electrostatic configuration
(ionic bonding)

Answer 5

• they have a full outer shell
• they do not react easily or at all
• elements in other groups do not have full outer shells

Question 6

electrostatic attraction meaning

Answer 6

force experienced by oppositely charged particles.

Question 7

What are the properties of ionic bonding

Answer 7

high melting and boiling point
high solubility in water
low (solid) and high conductivity (molten)

Question 8

why is there high melting/boiling points in ionic bonding

Answer 8

Strong electrostatic attractions between oppositely charged particles in all directions.

Requires a lot of energy needed to overcome strong attraction

Question 9

High solubility in water in ionic bonding

Answer 9

Water molecules can break the electrostatic attraction between ions

Question 10

conductivity in ionic bonding

Answer 10

solids ions have a low conductivity because they are in fixed positions

High conductivity as liquid/ gas ions are free to move

Question 11

recap questions (ionic bonding)

1. explain why the melting point of sodium chloride is high
2. explain why sodium chloride can dissolve in water
3. Why does sodium chloride have the formula NaCl and not NaCl2

Answer 11

1. There are strong electrostatic attractions between the P+N ions, takes a lot of heat to overcome them
2. The partial positive hydrogen atoms of water are attracted to the Cl⁻ ions, and the partial negative oxygen atoms are attracted to the Na⁺ ions, leading to dissociation
3. because it represents a 1:1 ratio of sodium ions to chloride ions

Question 12

Predict the formula of the following ionic compounds :
Potassium bromide
Lithium oxide
Calcium oxide

Answer 12

KBr
Li2O
CaO

Question 13

strength of ionic bonds

Answer 13

bigger charge = stronger bond
smaller size = stronger bond

Question 14

What type of atoms usually participate in covalent bonding

Answer 14

non-metals

Question 15

How is a covalent bond formed

Answer 15

by sharing an electron between atoms

Question 16

from which energy level do the electrons in covalent bonds come

Answer 16

outer energy level

Question 17

what is a dative covalent bond

Answer 17

a bond where there is 1 pair of shared electrons between two atoms

Question 18

what type of bond is formed when 2 pairs of electrons are shared

what type of bond if formed when 3 pairs of electron are shared

Answer 18

double bond

triple bond

Question 19

bond strength and bond length
H-F vs H-Br
which is stronger

Answer 19

As the bond length increases – the bond strength decreases

The bond length of bromine is longer because it’s under fluorine in the periodic table. Flourine bond length is shorter.

Meaning, fluorine is stronger because the bond length is shorter

Question 20

Which bond is stronger C=O or C-O? How do you know?

Answer 20

The first one is stronger because it is a double bond. It is shorter.

Question 21

Tehedral shape of organic compounds

Answer 21

• Electrons position themselves as far away from each other as possible

Question 22

properties of simple covalent bond and why?

Answer 22

LOW MELTING AND BOILING POINT
- covalent structures contain intermolecular forces. This is the force between molecules is weak so not much energy needed to melt
(they are usually gases in room temperature only few liquids)

DOES NOT CONDUCT ELECTRICITY
- no have a charge, remains neutral
- they can not move around, they are held in a covalent bond with a hydrogen atom

Question 23

Giant covalent compounds
What are the allotropes of carbon

Answer 23

Diamond, graphite, jewellery and pencils

Question 24

Giant covalent compounds
Diamond

Answer 24

• 4 strong covalent bonds per carbon
• High melting and boiling point - (requires lots of energy to break strong covalent bonds)
• Doesn’t conduct electricity - (no charged particles that can move)

Question 25

Graphite

Answer 25

• 3 strong covalent bonds per carbon
• High melting and boiling point - (requires lots of energy to break strong covalent bonds)
• Conducts electricity
• Slippery - (weak intermolecular forces between layers which can slide over each other)

Question 26

what type of atoms participate in metallic bonding

Answer 26

only metals

Question 27

what are the properties of metallic bonding

Answer 27

• conducts electricity
  Delocalised electrons that can move and carry the current
• high melting and boiling points
  Strong electrostatic attraction between delocalised electrons and (p) metal ions, require lots of energy to break
• Malleable (bent into shapes)
  Layers of ions which can slide over each other

Question 28

what happens in metallic bonding

Answer 28

Metals lose electrons to become positive metal ions. (electrons are delocalised)

Question 29

Why do metals conduct electricity

Answer 29

Has delocalised electrons that can move

Question 30

what is a delocalised electron

Answer 30

An electron not in a shell around an atom, it is free to move throughout the structure

Question 31

name some properties of metals

Answer 31

Conducts electricity, hard, dense, high melting point