Chapter 5

Question 1

How many electrons can fill the first energy level?

Answer 1

Two electrons fill the first energy level

Question 2

How many electrons can fill the second energy level?

Answer 2

Eight electrons can fill the second energy level

Question 3

How many electrons can fill the third energy level?

Answer 3

Eighteen electrons can fill the third energy level

Question 4

How many electrons can fill the fourth energy level?

Answer 4

Thirty two electrons can fill the fourth energy level

Question 5

What is the general formula for number of electrons

Answer 5

The general formula for number of electrons is 2n^2

Question 6

How many sub shells are there and what are their names?

Answer 6

There are four sub shells called: s,p, d and f.

Question 7

Definition of an atomic orbital

Answer 7

And orbital is a region around the nucleus that can hold up to 2 electrons with opposite spins

Question 8

What shape is an S orbital

Answer 8

And S orbital is spherical

Question 9

What shape is a p orbital

Answer 9

Appeal battle is dumb bell shaped

Question 10

How many orbitals are there in an S subshell and how many electrons can an s sub shell hold ?

Answer 10

An s subshell has one orbital this can hold 2 electrons

Question 11

How many orbitals does a p sub shell have and how many electrons can a p subshell hold?

Answer 11

A p sub shell has three orbitals thus can hold six electrons

Question 12

How many orbitals does a D subshell have and how many electrons can it hold?

Answer 12

A D subshell has five orbitals thus can hold 10 electrons

Question 13

When is filling orbitals in the same energy level should you occupy singly or pair first?

Answer 13

For all the tools in the same energy level occupy singly before pairing

Question 14

How do you write a shorthand electron configuration?

Answer 14

Write a shorthand electron configuration by putting the symbol of the previous noble gas in square brackets then the outer electron shells next to it

Question 15

Which subshell is the exception to the rule?

Answer 15

The 4S subshell is an exception because it is filled before the 3-D subshell as it is at low energy

Question 16

Definition of isoelectronic

Answer 16

I saw electronic – two ions that possess the same electronic configuration

Question 17

Definition of ionic bonding

Answer 17

Ionic bonding is the electrostatic attraction between positive and negative ions

Question 18

What do ionic compounds look like?

Answer 18

And it compounds from giant ionic lattices as charged ions attract oppositely charged ions in all directions

Question 19

Why are ionic compounds solid at room temperature?

Answer 19

Ionic compounds are solid at room temperature as there is insufficient energy to overcome the electrostatic forces between oppositely charged ions in the lattice

Question 20

Why do ionic compounds have high melting and boiling points

Answer 20

Ionic compounds have high melting points and boiling points because lots of energy is needed to overcome the electrostatic forces of attraction between oppositely charged ions in all directions. Ionic compounds with greater charges have higher melting and boiling points

Question 21

Are ionic compounds soluble?

Answer 21

Ionic compounds are soluble in polar solvents such as water as the polar molecules are Attracted to the irons and pull them away from the lattice causing them to dissolve

Question 22

Do ionic compounds conduct electricity?

Answer 22

Ionic compounds conduct electricity when molten or dissolved as the ions are free to move as mobile charge carriers

Question 23

Definition of a covalent bond

Answer 23

A covalent bond is strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 24

Covalent bonding which elements are exceptions to the octet rule?

Answer 24

Boron, Phosphorus, sulphur and chlorine are exceptions to the octet rule

Question 25

What covalent molecule does boron form that is an exception to the octet rule?

Answer 25

Boron forms BF3

Question 26

What covalent molecules does Phosphorus form that is an exception to the octet rule?

Answer 26

PF3 and PF5

Question 27

What covalent molecules does Sulfur form that is an exception to the octet rule?

Answer 27

SF2, SF4 and SF6

Question 28

What covalent molecules does Chlorine form that is an exception to the octet rule?

Answer 28

ClF, ClF3, ClF5 and ClF7

Question 29

What is a dative covalent bond?

Answer 29

A dative covalent bond is where both electrons are donated from one atom

Question 30

What is average bond enthalpy

Answer 30

Average bond enthalpy is a measurement of covalent bond strength. The larger the bond enthalpy the stronger the bond