3.1.3 Bonding

Question 1

What shape molecule has two bonding pairs and no lone pairs?

Answer 1

Linear

Question 2

What shaped molecule had 3 bonding pairs and 0 lone pairs?

Answer 2

Trigonal planar

Question 3

What shaped molecule had 2 bonding pairs and 1 lone pair

Answer 3

Bent (v- shape)

Question 4

What shaped molecule is 4 bonding pairs and 0 lone pairs?

Answer 4

Tetrahedral

Question 5

What shaped molecule has 3 bond pairs and 2 lone pair of electrons?

Answer 5

Trigonal pyramidal

Question 6

What shaped molecule had 2 bonding pairs and 2 lone pairs of electrons?

Answer 6

Bent (v- shape)

Question 7

What shaped molecule has 5 bonding pairs and 0 lone pairs of electrons?

Answer 7

Trigonal bipyramidal

Question 8

What shaped molecule has four bonding pairs and 1 lone pair of electrons?

Answer 8

Trigonal pyramidal/ seesaw

Question 9

What shaped molecule has 3 binding electrons and 2 lone pairs?

Answer 9

Trigonal planar/ t- shape

Question 10

What shaped molecule has 6 bonding electrons and 0 lone pairs?

Answer 10

Octahedral

Question 11

What shape has 5 bonding pairs and 1 lone pair?

Answer 11

Square pyramidal

Question 12

What shaped molecule has 4 bonding pairs and 2 lone pairs of electrons?

Answer 12

Square planar

Question 13

What is the definition for electron negativity?

Answer 13

How easily an element it functional group can attract electrons

Question 14

What are the four most electronegative elements?

Answer 14

Fluorine
Oxygen
Nitrogen
Chlorine

Question 15

In ionic bonding, what charge does the non metal have?

Answer 15

Negative

Question 16

What force attracts positive and negative ions?

Answer 16

Electrostatic attraction

Question 17

What are three properties of ionic compounds?

Answer 17

High melting point
Poor electrical conductivity (unless molten or dissolved)
Soluble in polar liquids eg water

Question 18

What does covalent bonding occur between?

Answer 18

Non metals and non- metals

Question 19

What is the definition for a covalent bond?

Answer 19

The electrostatic force of attraction between shared electrons and the neucleus

Question 20

What is the octet rule?

Answer 20

Where r bonded atoms achieve 8 electrons in the outer shell to achieve stability

Question 21

Which diagram can present a covalent bond?

Answer 21

Dot and cross diagram

Question 22

What are the five exceptions of the octet rule? (And how many electrons do they have instead)

Answer 22

Boron Triflouride (six)
Sulfur hexaflouride (12)
Phosphorus Pentachloride(10)
Chlorine Triflouride (6)
Sulphur Tetrafluoride (8)

Question 23

What is the definition for dative covalent bonding?

Answer 23

A covalent bond in which both shared electrons come from the same atom

Question 24

How is a dative covalent bond shown in a stick diagram?

Answer 24

An arrow pointing at the atom that is not sharing any of its own electrons

Question 25

What two structures can covalent structures be found?

Answer 25

Simple molecular Giant covelant

Question 26

What is the definition for electronegativity?

Answer 26

The ability of an atom to attract bonding electrons in a covalent bond

Question 27

What is a permanent dipole?

Answer 27

Where there is a small charge difference across a molecule but not enough for an ionic bond

Question 28

Why might a molecule with polar bonds not be polar?

Answer 28

It is symeytrical

Question 29

What is polarity determined by

Answer 29

The shape of molecule and electronegativity of atoms

Question 30

What force is responsible for melting and boiling point ?

Answer 30

Intermolecular

Question 31

What do covalent bonds effect?

Answer 31

Chemical reactions

Question 32

What is a vanderwaal force?

Answer 32

A force between all molecules caused by induced dipole-dipole interactions.

Question 33

How does an induce dipole-dipole interaction occur?

Answer 33

Electrons move to one side of molecule Creates a slight charge difference across molecule Attracts the electrons of the molecule next to it and the one next to that ext.

Question 34

T or F: Polar solute is soluble in polar solution

Answer 34

T

Question 35

Why can polar substances not dissolve in non-polar substances?

Answer 35

They have a different strength of intermolecular forces (permanent and induced dipole interactions) so the permanent dipole interactions can’t be broken by the induced dipoles therefore they cannot dissolve

Question 36

What three bonds allow for hydrogen bonding?

Answer 36

N-H F-H O-H

Question 37

Why does hydrogen bonding occur

Answer 37

The electrons from the hydrogens in a F-H, N-H or O-H move away from the hydrogen creating a dipole, this causes the hydrogen to attract the lone pair of electrons from another O, N or F atom.

Question 38

What property of water is unusual due to hydrogen bonding

Answer 38

Ice is less dense that water

Question 39

What is the definition for metallic bonding?

Answer 39

A lattice of closely packed, positive ions in a sea of delocalised electrons

Question 40

What element has the highest melting and boiling point on period 3? And why

Answer 40

Silicon, it forms a covalent lattice which means that it needs to have its covalent bonds broken before it can be melted.

Question 41

What three types of bonding occur in period 3and with what elements?

Answer 41

Metallic bonding- sodium, magnesium, Aluminium Giant covalent- silicone Simple covalent- phosphorus, Sulfur, chlorine

Question 42

Name the elements in period 3

Answer 42

Sodium Magnesium Aluminium Silicon Phosphorus Chlorine Argon