Unit One Stuff

Question 1

High electronegativity is likely to do what to electrons

Answer 1

Attract

Question 2

What is electronegativity

Answer 2

The attraction an element has for the shared pair of electrons in a covalent bond

Question 3

Electronegativity: trends ACROSS period

Answer 3

Increases as number of protons increases

Question 4

Electronegativity: tends DOWN a group

Answer 4

Electronegativity decreases due to increase in shells,

Question 5

Difference in electronegativity that is lower than 0.3 means that:

Answer 5

PURE COVALENT,

Question 6

Electronegativity difference between 0.3 and 1.8 means

Answer 6

Polar covalent

Question 7

Electronegativity difference greater than 1.8 means it’s

Answer 7

Ionic

Question 8

Covalent radius is

Answer 8

Half the distance between the nuclei of two covalently bonded atoms

Question 9

Covalent Bond length can be calculated by

Answer 9

Adding together the radii of the two atoms bonding

Question 10

Trends in covalent radius ACROSS a period

Answer 10

Decreases due to an increase in protons therefore tighter pull

Question 11

Trends in covalent radius DOWN a group

Answer 11

Number of Electron shells increases therefore atoms get bigger

Question 12

Which larger ionic radius Cl or Cl-

Answer 12

Cl- bcs it has an electron arrangement of 2,8,8 meaning it has 18 electrons which is more difficult for the 17 protons to hold tightly so it is bigger

Question 13

Ionisation energies, endothermic or exothermic

Answer 13

Endothermic

Question 14

First ionisation energy is the energy require to

Answer 14

Remove one mole of electrons from one mole of atoms in the gas phase

Question 15

Ionisations energies are WHAT when an electron is removed from a full shell

Answer 15

MUCH MUCH MUCH LARGER

Question 16

Why are ionisation energies greater when removing electrons from a full shell

Answer 16

Full shells are more stable and shells closer to the nucleus feel a stronger pull from the nucleus

Question 17

Trends in ionisation energy ACROSS a period

Answer 17

It increases, due to the number of protons increasing whilst shielding remains constant

Question 18

Trends in ionisation energy DOWN a group

Answer 18

Decreases, as going down a group the number of electron shells increases leading rn the outer electrons being held weakly

Question 19

Covalent networks:

Answer 19

Don’t conduct and have high melting points, think a rigid net

Question 20

Covalent molecule:

Answer 20

Don’t conduct and have low melting point, think a sploogy goo

Question 21

Ionic:

Answer 21

High melting point, conducts as liquid or in a solution

Question 22

Name of the force of attraction given to lone atoms and molecules

Answer 22

Van der Waal forces

Question 23

LDF occur when:

Answer 23

The movement of electrons in an atom leading to one side being positive the other being negative, thus has an affect on nearby atoms

Question 24

LDF, more electrons mean

Answer 24

Stronger force

Question 25

How LDF form: Dipole is

Answer 25

A charge difference

Question 26

How LDF form: temporary dipole is

Answer 26

Temporary charge difference

Question 27

How do (temporary) dipoles form

Answer 27

When electron happen to move to one side of a molecule

Question 28

Induced is when

Answer 28

Another atom/molecule approaches a dipole, they become induced, they are attracted to eachother. this is LDF

Question 29

Description of Metallic structure

Answer 29

Positive metal ions surrounded by a sea of negative electrons, gd at conducting head and electricity due to DELOCALISED ELECTRONS

Question 30

3 forms (allotropes) of carbon

Answer 30

Diamond, graphite and fullerene

Question 31

Diamond is:

Answer 31

Carbon atoms making covalent bonds to 4 other carbons, doesn’t conduct electricity

Question 32

Graphite SHEETS stay together due to?

Answer 32

LDF

Question 33

Binding and structure of Graphite

Answer 33

Covalent network

Question 34

Fullerene are

Answer 34

The football things, molecules of carbon

Question 35

Polar molecules have permanent dipoles due to

Answer 35

Polar bonds in the molecules AND the shape of the molecule learning to bond polarity’s being unsymmetrical

Question 36

Strength of P.d to P.d LDF and H binding

Answer 36

1 H bonding, 2 p.d to p.d, 3 LDF

Question 37

Hydrogen binding occurs when

Answer 37

Hydrogen bonds with F, N or O within a molecule

Question 38

IMF (Van see Waal) influence properties in molecules such as:

Answer 38

Melting & boiling pts, volatility (evaporate), viscosity (how easily it pours), solubility

Question 39

In H-bonding the more -OH or -NH groups lead to

Answer 39

Higher melting & boiling pts

Question 40

Solubility “like dissolves like” means

Answer 40

Polar molecules are soluble in POLAR solvents, Non polar molecules are soluble in NON POLAR solvents

Question 41

Ox agent is;

Answer 41

A chemical which causes something else to be oxidised, it causes electron loss by gaining the electron for itself

Question 42

Reducing Agents :

Answer 42

Causes something else to be reduced i.e gd at LOSING electrons

Question 43

Standard solution

Answer 43

Solution of accurately known concentration

Question 44

CHROMA TOGRAPHY: Retention time is affected by

Answer 44

size of molecule and polarity (more polar linger time)