The name's Bond. Chemical Bond.

Question 1

What type of elements are Simple Covalent bonds between? [1]

Answer 1

Simple Covalent bonds are between non-metals. [1]

Question 2

Describe the structure of Simple Covalent bonds. [2]

Answer 2

A Simple Covalent bond’s structure is comprised of small, simple molecules. The structure is held together by weak intermolecular forces of attraction. [2]

Question 3

State and describe the conductivity of Simple Covalent bonds. [3]

Answer 3

Simple Covalent bonds DO NOT CONDUCT [1] because they HAVE NO DELOCALISED ELECTRONS [1] to CARRY CHARGES THROUGH THE STRUCTURE [1].

Question 4

State and describe the melting point of Simple Covalent bonds. [3]

Answer 4

Simple Covalent bonds have a RELATIVELY LOW MELTING POINT [1] because the WEAK INTERMOLECULAR FORCES [1] DON’T REQUIRE MUCH ENERGY TO BREAK [1].

Question 5

True or False?
In Simple Covalent bonds, an element gives away an electron/electrons to another element. [1]

Answer 5

False. In Simple Covalent bonds, elements share electrons. [1]

Question 6

What type of elements are Ionic bonds between? [1]

Answer 6

Ionic bonds are between metals and non-metals. [1]

Question 7

Describe the structure of Ionic bonds. [3]

Answer 7

An Ionic bond’s structure is a lattice structure that is comprised of positive metal ions and negative non-metal ions. [3]

Question 8

State and describe the conductivity of Giant Ionic bonds. [3]

Answer 8

Giant Ionic bonds ONLY CONDUCT [1] WHEN MOLTEN OR AQUEOUS [1] BECAUSE THE IONS ARE FREE TO MOVE [1].

Question 9

State and describe the melting point of Giant Ionic bonds. [4]

Answer 9

Giant Ionic bonds have a HIGH MELTING POINT [1] because the ELECTROSTATIC FORCES OF ATTRACTION BETWEEN THE POSITIVE METAL IONS AND NEGATIVE NON-METAL IONS [2] REQUIRE A LOT OF ENERGY TO BREAK [1].

Question 10

True or False?
In Ionic bonds, an element shares an electron/electrons with another element. [1]

Answer 10

False. In Ionic bonds, elements transfer electrons. [1]

Question 11

What type of elements are Metallic bonds between? [1]

Answer 11

Metallic bonds are between metals. [1]

Question 12

Describe the structure of Metallic bonds. [2]

Answer 12

Metallic bonds are comprised of a ‘sea’ of delocalised electrons. [2]

Question 13

State and describe the conductivity of Giant Metallic bonds. [3]

Answer 13

Giant Metallic bonds CONDUCT ELECTRICITY [1] because they have a SEA OF DELOCALISED ELECTRONS [1] that can CARRY CHARGES THROUGHOUT THE ENTIRE STRUCTURE [1].

Question 14

State and describe the melting point of Giant Metallic bonds. [4]

Answer 14

Giant Metallic bonds have a HIGH MELTING POINT [1] because the STRONG ELECTROSTATIC FORCES OF ATTRACTION BETWEEN THE NEGATIVE DELOCALISED ELECTRONS AND THE POSITIVE METAL IONS [2] REQUIRE A LOT OF ENERGY TO BREAK [1].

Question 15

True or False?
In metallic bonds, elements share electrons. [1]

Answer 15

True. [1]

Question 16

Describe the structure of a Giant Covalent bond. [1]

Answer 16

A Giant Covalent bond’s structure is a giant lattice structure.

Question 17

State and describe the conductivity of Giant Covalent bonds. [4]

Answer 17

Giant Covalent structures GENERALLY DO NOT CONDUCT ELECTRICITY [1] because they HAVE NO OVERALL CHARGE [1]. GRAPHITE IS AN EXCEPTION [1]; it can conduct because it HAS DELOCALISED ELECTRONS [1].

Question 18

State and describe the melting point of Giant Covalent bonds. [3]

Answer 18

Giant Covalent bonds have VERY HIGH MELTING POINTS [1] because there are A LOT OF STRONG COVALENT BONDS [1] that REQUIRE A LOT OF ENERGY TO BREAK [1].

Question 19

Even though Giant Covalent bonds have weak intermolecular forces, it requires a lot of energy to melt Giant Covalent bonds. Why is this? [2]

Answer 19

This is because Giant Covalent bonds have strong Covalent bonds holding the molecules together, but they have weak intermolecular forces between molecules.

Question 20

A bond between Magnesium and Oxygen is a __________ bond. [1]

Answer 20

Ionic [1]

Question 21

A bond between Chlorine and Hydrogen is a __________ bond. [1]

Answer 21

Covalent [1]

Question 22

What is an Atomic Number? [1]

Answer 22

Atomic Number is the number of protons in the nucleus of an atom. [1]

Question 23

What is a Mass Number? [1]

Answer 23

The total number of protons and neutrons in a nucleus. [1]

Question 24

What is the mass of a proton, neutron, and electron? [3]

Answer 24

Proton - 1 [1]
Neutron - 1 [1]
Electron - 1/2000 [1]

Question 25

What is the charge of a proton, neutron, and electron? [3]

Answer 25

Proton = +1 [1]
Neutron = 0 [1]
Electron = -1 [1]

Question 26

What is the trend in properties in Group 1 (Alkali Metals) of the periodic table as you go down the group (melting point, boiling point)? [4]

Answer 26

The melting point decreases as you go down the group. [2]
The boiling point decreases as you go down the group. [2]

Question 27

What is the trend in properties in Group 7 of the periodic table as you go down the group (melting point, boiling point)? [4]

Answer 27

The melting point increases as you go down the group. [2]
The boiling point increases as you go down the group. [2]

Question 28

What is the trend in properties in Group 0 of the periodic table as you go down the group (melting point, boiling point)? [4]

Answer 28

The melting point increases as you go down the group. [2]
The boiling point increases as you go down the group (except for caesium). [2]

Question 29

What is the trend in reactivity in Group 1 of the periodic table as you go down the group? [2]

Answer 29

The reactivity gets more vigorous as you go down the group [2].

Question 30

Describe Group 1’s reactivity with water (word and symbol equation) [8]

Answer 30

Lithium + Water = Hydrogen + Lithium Hydroxide

2Li + 2H`2O = H’2 + LiOH

Question 31

Describe what happens when potassium reacts with fluorine to produce potassium fluoride. [4]

Answer 31

• Potassium loses one electron [2]
• Fluorine gains one electron [1]
• Potassium forms positive ion [1]
• Fluorine forms negative ion [1]

Question 32

How many electrons are there in each shell of a chloride ion? [3]

Answer 32

2, 8, 8 [3]

Question 33

Describe the structure and bonding of sodium chloride. [4]

Answer 33

• giant lattice
• ionic / contains ions [1]
• sodium (positive), chloride (negative) ions
• Electrostatic force of attraction