Electrons, Bonding and Structure full module

Question 1

What are electron shells made up of?

Answer 1

Sub-shells and orbitals

Question 2

What do electrons move around the nucleus in?

Answer 2

shells (energy levels)

Question 3

What is the name of the number given to shells?

Answer 3

Principle quantum number

Question 4

What are shells divided into and what are there 4 names

Answer 4

Subshells, S P D and F

Question 5

What does each subshell have a different number of?

Answer 5

orbitals

Question 6

How many electrons can fit into 1 orbital?

Answer 6

2

Question 7

How many orbitals does the S and P subshell have speperatly?

Answer 7

S:1 P:3

Question 8

What shape is the S orbitall?

Answer 8

spherical

Question 9

What shape is the P orbital?

Answer 9

Dumbell

Question 10

what is the electron configuration of potassium (K) (19e’s)

Answer 10

1s2 2s2 2p6 3s2 3p6 4s1

Question 11

How are ions formed?

Answer 11

When electrons are transferred from one atom to another so as to have a full outer shell, they can be positively or negatively charged.

Question 12

What holds ions together?

Answer 12

electrostatic attraction

Question 13

What is an ionic bond?

Answer 13

an electrostatic attraction between two oppositly charged ions

Question 14

What diagram shows ionic bonding?

Answer 14

dot and cross diagrams

Question 15

Do ionically bonded substances conduct electrisity? why

Answer 15

Yes when molten or dissolved as the ions can move and carry a charge

Question 16

What type of mp and bp do ionic comounds have? why

Answer 16

High as the giant ionic lattices are held together by strong electrosatic forces that take lots of energy to overcome.

Question 17

Why do ionic compunds dissolve?

Answer 17

As water is polar so part of the molecule is attracted the the water and part of it pull it away causing it to dissolve

Question 18

What are molecules nd what holds them together?

Answer 18

they are two or more atoms covalently bonded together

Question 19

what is covalent bonding?

Answer 19

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

Question 20

What is dative covalent bonding?

Answer 20

When both electrons in a bond come from one atom

Question 21

What repels more bonded pairs or lone pairs?

Answer 21

lone pairs

Question 22

In molecule shapes where is the greatest angle

Answer 22

between lone pairs

Question 23

If a molecule has 2 bonded pairs and 0 lone pair what is the bond angle and shape of the molecule?

Answer 23

linear 180

Question 24

if a molecule has 3 bonded pairs and 0 lone pair what is the bond angle and shape of the molecule?

Answer 24

trigonal planar 120

Question 25

if a molecule has 3 bonded pairs and 1 lone pair what is the bond angle and shape of the molecule?

Answer 25

bent and angle<120

Question 26

if a molecule has 4 bonded pairs and 0 lone pair what is the bond angle and shape of the molecule?

Answer 26

tetrahedral 109.5

Question 27

if a molecule has 4 bonded pairs and 1 lone pair what is the bond angle and shape of the molecule?

Answer 27

pyramidal angle<109.5

Question 28

if a molecule has 4 bonded pairs and 2 lone pair what is the bond angle and shape of the molecule?

Answer 28

bent angle<109.5

Question 29

if a molecule has 5 bonded pairs and 0 lone pair what is the shape of the molecule?

Answer 29

trigonal bipyramidal

Question 30

if a molecule has 6 bonded pairs and 0 lone pair what is the bond angle and shape of the molecule?

Answer 30

octahedral 90

Question 31

what is electronegativity

Answer 31

an atom's ability to attract the electron pair in a covalent bond

Question 32

what is the most electronegative molecule and the top 3 after

Answer 32

Flourine then oxygen, nitrogen and chlorine

Question 33

What is electronegativity measured in?

Answer 33

the pauling scale

Question 34

why may a covalent bond be polarised?

Answer 34

difference in electronegativity

Question 35

How is a bond polar/

Answer 35

between two atoms of different electronegativity when the bonding electrons are pulled towards the more electronegative atom

Question 36

What is a dipole?

Answer 36

a shift in electron density in a bond

Question 37

What is caused by a polar bond?

Answer 37

a permanent dipole

Question 38

What makes a bond more polar?

Answer 38

a greater difference in electron density

Question 39

Give an example of when a covalent bond is non polar?

Answer 39

between diatomic gases eg H2 Cl2

Question 40

How is charge arranged in polar molecules?

Answer 40

unevelenly

Question 41

What happens if polar bonds are arranged symmetrically

Answer 41

The dipoles cancel out and the bond is non-polar an example is carbon dioxide

Question 42

What bonds are truely covalent?

Answer 42

Only those between a single element.

Question 43

How can you use electronegativity to predict what type of bond will occur between 2 atoms?

Answer 43

The higher the difference in electronegativity the more ionic it becomes

Question 44

How strong are intermolecular forces?

Answer 44

Very weak. weaker than all types of bonding

Question 45

Are all compounds covalent or ionic?

Answer 45

No, most compunds are inbetween ionic and covalent

Question 46

what are the 3 intermolecular forces?

Answer 46

1. Induced dipole-dipole forces (Lodnon forces) 2. Permanent dipole-dipole interations 3.Hydrogen bonding

Question 47

What is induced dipole-dipole forces (London forces)?

Answer 47

Electrons in a charged cloud are always moving, any any particular moment they are more likely to be on one side of an atom then the other. This causes a tempory dipole.

Question 48

What atoms do induced dipole-dipole forces happen in

Answer 48

All atoms even noble gases

Question 49

What can induced dipole-dipole forces cause?

Answer 49

A neighbouring atom to experience another induced dipole in the opposite direction, this causes a chain of dipoles in atoms near eachover.

Question 50

What does the stronger induced dipole dipole forces cause? and why?

Answer 50

Higher bp and mp. Because the larger electron cloud has more intermolecular forces which need to be broken in order to boil a substance.

Question 51

What are permanent dipole-dipole interations?

Answer 51

Slightly negative and positive charges on polar molecules causing weak electrostatic forces of attraction between molecules.

Question 52

What is the strongest intermolecular force?

Answer 52

Hydrogen bonding

Question 53

What can hydrogen bonding occur between?

Answer 53

Hydrogen and Flourine, Nitrogen or Oxygen.

Question 54

Why does hydrogen bond to Floruine (or oxygen or nitrogen)

Answer 54

as hydrgoen has a high charge density because it is so small and flourine is very electronegative. The bond is so polarised that a weak bond between the hydrogen of one molecule and a long pair of electrons on the flourine in another molecule.

Question 55

When drawing molecules what does a straight line show us?

Answer 55

The bonds and their atoms lie on the plane of the page

Question 56

When drawing molecules what does a solid wedge show us?

Answer 56

The bond and its atom is coming out of the plane of the page