Unit 2 - BPA

Question 1

Orbital definition

Answer 1

A region in an atom that can hold up to two electrons with opposite spin

Question 2

Principle quantum number

Answer 2

Shell number

Question 3

Electron shell definition

Answer 3

Group of atomic orbitals with the same principle quantum number

Question 4

s-orbital shape

Answer 4

sphere

Question 5

p-orbital shape

Answer 5

dumbell

Question 6

Are 4s or 3d electrons removed first

Answer 6

4s

Question 7

What type of forces hold the particles together in ionic bonding?

Answer 7

Electrostatic forces of attraction

Question 8

What type of elements is ionic bonding between?

Answer 8

Non-metals and Metals

Question 9

What type of elements is covalent bonding between?

Answer 9

Metals

Question 10

Covalent bonding definition

Answer 10

The strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms

Question 11

How many covalent bonds does Hydrogen make?

Answer 11

1

Question 12

How many covalent bonds does Carbon make?

Answer 12

4

Question 13

How many covalent bonds does Nitrogen make?

Answer 13

3

Question 14

How many covalent bonds does Oxygen make?

Answer 14

2

Question 15

Lone pair definiton

Answer 15

An unpaired pair of electrons

Question 16

Bond enthalpy definition

Answer 16

The energy required to break a particular covalent bond in one molecule of a gaseous molecule

Question 17

Larger bond enthalpy

Answer 17

Stronger bond

Question 18

Linear bond angle

Answer 18

180

Question 19

Trigonal planar bond angle

Answer 19

120

Question 20

Tetrahedral bond angle

Answer 20

109.5

Question 21

Octahedral bond angle

Answer 21

90

Question 22

Electronegativity definition

Answer 22

The measure of an atoms ability to attract a pair of electrons towards itself

Question 23

Does electronegativity increase or decrease from left to right and down to up?

Answer 23

Increase

Question 24

Ionic bonding definition

Answer 24

Electrostatic attraction between positive and negative ions

Question 25

Order of intermolecular forces

Answer 25

Induced dipole-dipole interactions < Permanent dipole-dipole interactions < Hydrogen bonding

Question 26

Why is ice less dense than liquid water?

Answer 26

Hydrogen bonds are longer than Covalent bonds, causing an open lattice structure to form

Question 27

Why does water have a higher melting and boiling point than expected?

Answer 27

Hydrogen bonds are stronger than other intermolecular forces

Question 28

Hydrogen bond defininiton

Answer 28

A strong dipole-dipole interaction between an electron deficient hydrogen atom on one molecule and a lone pair of electrons on a very electronegative atom on a different molecule