Electrons and Bonding

Question 1

What is the shell number (energy level number) called?

Answer 1

The principal quantum number

Question 2

What are shells made up of?

Answer 2

Atomic orbitals

Question 3

What is an atomic orbital?

Answer 3

A region around the nucleus that can hold up to two electrons with opposite spins

Question 4

How many electrons can an orbital hold?

Answer 4

One or two

Question 5

What are the different types of orbitals?

Answer 5

S
P
D
F

Question 6

What is an s orbital?

Answer 6

An electron cloud within the shape of a sphere

Question 7

What shape is a p orbital?

Answer 7

An electron cloud within the shape of a dumb bell

Question 8

How many p orbitals are there?

Answer 8

Three separate ones all at right angles to one another

Question 9

What happens to s orbitals as the shell number increases?

Answer 9

Their radius increases

Question 10

What happens to p orbitals as the shell number increases?

Answer 10

The p orbital gets further from the nucleus

Question 11

How many d orbitals are there?

Answer 11

Five

Question 12

How many f orbitals are there?

Answer 12

Seven

Question 13

What are sub-shells?

Answer 13

Orbitals of the same type grouped together

Question 14

How do orbitals fill?

Answer 14

In order of increasing energy

Question 15

What must two electrons have to share the same orbital?

Answer 15

Opposite spins

Question 16

What do the opposite spins of the electrons do?

Answer 16

Counteract the repulsion between the negative charges of two electrons

Question 17

What is special about the 4s and 3d sub-shells?

Answer 17

4s fills before 3d

4s empties before the 3d

Question 18

What is ionic bonding?

Answer 18

The electrostatic attraction between positive and negative ions

Question 19

Describe shells

Answer 19

Regarded as energy levels

The energy increases as the shell number increases

Question 20

I which directions does each ion attract?

Answer 20

All directions

Question 21

What is the structure of ionic compounds?

Answer 21

A giant ionic lattice

Question 22

How many ions is each ion surrounded by in a giant ionic lattice?

Answer 22

6

Question 23

Why are most ionic compounds solid at room temperature?

Answer 23

There is insufficient energy to overcome the strong electrostatic forces of attraction between the oppositely charged ions in the lattice

Question 24

What melting and boiling points do ionic compounds have?

Answer 24

High ones

Question 25

What makes the melting points higher for ionic lattices?

Answer 25

If they contain ions with greater ionic charges

Question 26

What is the nitrate ion?

Answer 26

NO3-

Question 27

What is the sulphate ion?

Answer 27

SO4 2-

Question 28

What is the carbonate ion?

Answer 28

CO3 2-

Question 29

What is the ammonium ion?

Answer 29

NH4+

Question 30

What is the hydroxide ion?

Answer 30

OH-

Question 31

What is the zinc ion?

Answer 31

Zn 2+

Question 32

What is the silver ion?

Answer 32

Ag +

Question 33

What is lattice energy?

Answer 33

Energy required to break bonds (electrostatic attractions) between a giant ionic lattice

Question 34

What is electro negativity?

Answer 34

A measure of the electron attracting power of an atom

Question 35

What does it mean if a molecule is polar

Answer 35

Uneven electron distribution creating a slight electronegative charge on the atoms

Question 36

Why is water a polar molecule?

Answer 36

Because Oxegyn has a higher electro negativity than hydrogen so the electrons are pulled closer to it in the covalent bond

Question 37

What is hydration energy?

Answer 37

The energy the water has for pulling apart the giant ionic lattice

Question 38

How is an ionic lattice pulled apart by water?

Answer 38

The water surrounds to ion and rips it off by sheer numbers

Question 39

What are spectator ions?

Answer 39

Ions which are not changed by the reaction

Question 40

What does hydrated mean?

Answer 40

Water molecules are trapped in the lattice

Question 41

What does anhydrous mean?

Answer 41

No water molecules trapped in the lattice

Question 42

What are lone pairs?

Answer 42

Electrons not bonded to anything

Question 43

Name six different shapes of atoms

Answer 43

``` Linear Trigonal Tetrahedral Trigonal pyramidal Trigonal bypiramidal Octahedral ```

Question 44

What is a dative covalent bond?

Answer 44

Where the pair of electrons in a covalent bond is provided by one atom

Question 45

Name three factors that affect electronegativity

Answer 45

Size No of protons "Shielding" (how many electrons surround the nucleus)

Question 46

What is the degree of angle on a trigonal planar?

Answer 46

120

Question 47

Why are there different shapes

Answer 47

Because electrons need the most amount of space to avoid repulsion