Chemical Bonding Unit 1

Question 1

7 main VSEPR types

Answer 1

Linear
Trigonal Planar
Tetrahedral
Triangular Pyramidal
Angular/Bent
Triangular Bi-Pyramidal
Octahedral

Question 2

Type and class

Answer 2

AX2
Linear

Question 3

Type and class

Answer 3

AX3
Trigonal Planar

Question 4

Type and class

Answer 4

AX4
Tetrahedral

Question 5

Type and class

Answer 5

AX3E
Triangular Pyramidal

Question 6

Type and class

Answer 6

AX2E2
Angular/Bent

Question 7

Type and class

Answer 7

AX2E
Bent

Question 8

Type and class

Answer 8

AXE3
Linear

Question 9

Type and class

Answer 9

AX6
Octahedral

Question 10

Type and class

Answer 10

AX5
Triangular Bi-Pyramidal

Question 11

Why do chemical bonds form?

Answer 11

To fill valence shell

Question 12

How many ways can an atom obtain a full valence, shell, and how?

Answer 12

They can either gain or lose electrons, which is known as ionic bonding

They can share electrons between atoms. This is covalent bonding.

Question 13

How do you determine if an atom shares electrons or transfers electrons

Answer 13

Through electronegativity, it’s a number that decides the desire, and Atom has for a pair of electrons

The larger the number the more Adam wants electrons

Question 14

How do you determine if a bond is ionic or covalent?

Answer 14

By looking at the difference between their electronegativities

Question 15

Electronegative chart

Answer 15

Question 16

When do ionic bonds form?

Answer 16

When electrons are transferred from one atom to another

Question 17

What is the strongest bond possible?

Answer 17

Ionic bonds

Question 18

What do ionic compounds form and not form?

Answer 18

They form crystals otherwise known as a crystal lattice

They don’t form molecules

Question 19

How are covalent bonds formed?

Answer 19

They’re formed when electrons are shared between atoms

Question 20

Ways for atoms to share electrons

Answer 20

When shared equally the bond is nonpolar

When shared unequally, the bond is polar

Question 21

How do you know which side of a bond is slightly negative and which side is slightly positive?

Answer 21

The atom that has the most electrons will become slightly negative

Question 22

How to draw E-dot diagrams

Answer 22

Use the octet rule where atoms want eight valence electrons

Question 23

Four steps in drawing an E-dot diagram

Answer 23

1.) how many atoms of each element are in the molecule

2.) figure out which atoms are connected.

3.) determine the number of dots

4.) decide where the dots go.

Question 24

What is a double bond?

Answer 24

When two pairs of electrons are shared

Question 25

Seven. Exceptions to the octet rule.

Answer 25

1.)H only needs two valence electrons. 2.) alkaline metals only need 2 3.) B and down only need six. 4.) Be only needs four. 5.) phosphorus can have up to 10 valence electrons. 6.) sulphur can have up to 12. 7.) sometimes tin will only need six.

Question 26

What is a resonance structure?

Answer 26

A structure used when no single structure adequately represents the molecule 

Question 27

VSEPR and what it means

Answer 27

Valence shell electron pair repulsion theory Pairs of electrons repel each other, in order to get as far apart as possible

Question 28

What is intermolecular attraction?

Answer 28

Attraction between different molecules Ex:

Question 29

What is intra-molecular attraction?

Answer 29

Attraction within the same molecule

Question 30

What is a dipole?

Answer 30

When one end of the molecule is slightly positive and the other end of the molecule is slightly negative

Question 31

What happens when a molecule has a slightly positive, charged a slightly negatively charged end

Answer 31

The molecule have a dipole-dipole attraction

Question 32

Which has a higher attraction and why

Answer 32

Left The bond is between hydrogen and oxygen

Question 33

What is an H bond?

Answer 33

An attraction between hydrogen from one molecule, and a molecule of nitrogen, oxygen, or fluorine from another

Question 34

How much stronger are hydrogen bonds than dipole dipole?

Answer 34

10 times stronger

Question 35

What are London forces?

Answer 35

The result of an unequal distribution of electrons in a molecule

Question 36

Where are London forces present?

Answer 36

In all molecules, but significant in nonpolar

Question 37

Types of intermolecular forces, and what they are known as

Answer 37

1.) H-bonds 2.) dipole-dipole 3.) London forces Known as Vander waals forces

Question 38

Does H2O or H2S have a higher boiling point and why

Answer 38

H2O because it has a hydrogen bond (NOF)