wording

Question 1

Trends Structure

Answer 1

Define factor
state the trend
what is happening to # of p and nuclear charge
where are e going
what does this mean for sheilding and dist from nucleus
what does this mean for factor

Question 2

Atomic Radii decreases

Answer 2

across the period

Question 3

Atomic increases

Answer 3

down a group

Question 4

electron are added to same shell

Answer 4

across a period

Question 5

e are added to new shells

Answer 5

down a period

Question 6

Electronegativity (def)

Answer 6

the measure of attraction between a nucleus and a bonding pair of e

Question 7

Electrongativity increases

Answer 7

across a period (left to right)

Question 8

Electronegativity decreases

Answer 8

down a group

Question 9

Atomic Radii (def)

Answer 9

total distance from the nucleus of an atom to the outermost orbital of its electron

Question 10

1st Ionisation energy (def)

Answer 10

the energy required to remove the least tightly bound electron from a mole of atoms in the gaseous state

Question 11

High Ionisation energy

Answer 11

takes a lot of energy to remove the outermost e

Question 12

Low Ionisation energy

Answer 12

takes a small amount of energy to remove outermost e

Question 13

1st ionisation energy increases

Answer 13

across a period

Question 14

1st ionisation energy decreases

Answer 14

down a group

Question 15

Once 1 e has been removed

Answer 15

more energy is needed to remove the second e

Question 16

Ionic Radius (def)

Answer 16

the radius of an ion

Question 17

Cations are (postive ions)

Answer 17

smaller in radii and smaller than their parent atom (if all the v electrons are removed there is one less occupied energy level with no change in nuclear charge)

Question 18

Anions are (negative ions)

Answer 18

larger in radii and are bigger than their parent atom (if there are more electrons in the valence level so there is greater e- to e- repulsion with no change in nuclear charge)

Question 19

Shape Template

Answer 19

number of e clouds around central atom
e are negatively charged and repel each other to maximize separation and minimize repulsion
parent arrangement and angle
Number of non bonding and bonding pairs
non bonding pairs contribute to shape but are not part of it
final shape

Question 20

Which atom is more electronegative

Answer 20

FONCl BrISCHP

Question 21

Solubility Def

Answer 21

The ability of a substance solute to dissolve (break up) in a given solute

Question 22

Exceptions in Electron Configuration are

Answer 22

Cu and Cr

Question 23

Ionisation Energy Factors-

Answer 23

The stronger the attraction of the nucleus to the electron, the more energy required to remove the electron.

Question 24

Electronegativity increase across a period due to

Answer 24

(atomic number) increasing positive charge due to increasing number of protons in the nucleus

Valence electrons across a period are in the same energy level which means

a decrease in atomic radius as valence electrons are pilled in closer due to strong electrostatic attraction

increase in first ionization energy- valence electrons are harder to remove

Question 25

Electronegativity decreases down a group due to

Answer 25

increasing distance of the valence electron shell from nucleus so electrostatic attraction is reduced increasing number of electron shells shields the nucleus increase in atomic size- less attractive forces pulling the valence e to the nucleus decreasing first ionization energy- less attraction between nucleus and valence e- easier to remove

Question 26

Shape Structure

Answer 26

1.Number of electron clouds 2.electron clouds repel around central atom “and maximise separation to minimise repulsion” 3.Parent shape 4. Angles 5.Number bonding and non bonding pairs 6.Non bonding pairs “contribute to shape but are not part of it”. 7.Shape

Question 27

Electron Repulsion wording

Answer 27

These electron clouds are negatively charged and mutually repel around the central atom to maximize separation and minimize repulsion

Question 28

Lone pairs in shape

Answer 28

contribute to the shape but are not part of it

Question 29

Intermolecular Bonds (def)

Answer 29

The forces between the molecules that are broken when a substance melts or evaporates

Question 30

Name the three types of intermolecular Bonds

Answer 30

Temporary Dipoles, Permanent Dipoles, Hydrogen Bonding

Question 31

Temp Dipoles occur in

Answer 31

all molecules

Question 32

Permanent Dipoles occur in

Answer 32

Polar Molecules

Question 33

Hydrodgen Bonds occur in

Answer 33

polar molecules with H bonded to O, F or N

Question 34

Solubility =

Answer 34

the ability of a substance(solute) to dissolve (break up) in a given solvent

Question 35

A solute will dissolve if:

Answer 35

solute-solvent forces ≥ solvent-solvent and solute-solute force

Question 36

Entropy Question Template

Answer 36

Entropy - degree of disorder or randomness Reactions will be spontaneous if total entropy change (system + surroundings) is positive. Entropy of system (ΔSsystem)– increasing or decreasing? Enthalpy of system (ΔH) - increasing or decreasing? Entropy of surroundings (ΔSsurroundings)– increasing or decreasing? Total entropy change – positive or negative?

Question 37

Polarity of a molecule template

Answer 37

The molecule is [shape] and is [symmetrical/asymmetrical]. In the __-___ bond ___ is more electronegative than ____. The electrons will spend more time at __ than___ so __ is slightly negative and ___ is slightly positive. Therefore the __-___ bond is [polar/nonpolar] As the molecule is is [symmetrical/assymetrical] the [dipoles cancel/ don’t cancel] and so the molecule is [polar/non polar].