Topic 1

Question 1

Occupied shells tells us

Answer 1

Period number

Question 2

Valence shell tells us the

Answer 2

Group number

Question 3

Emission spectra and the atom

Answer 3

When element is heated, electrons absorb energy and promoted to higher energy state (excited state)
When element relapses from excited to lower energy state (ground state), energy is released as electromagnetic radiation which we see as colour

Question 4

Bohr model

Answer 4

Electron in given orbit has constant energy
Electrons can only occupy fixed energy levels and not exist between two levels
Orbits of larger radii (further away from nucleus) means more energy

Question 5

How many electrons can a sub shell hold

Answer 5

2 in each orbital

Question 6

Orbital

Answer 6

Region of space in which up to two electrons are likely to be located

Question 7

How many electrons can p is shell hold

Answer 7

6

Question 8

How many electrons can d sub shell hold

Answer 8

10

Question 9

How many electrons can you hold in each orbital

Answer 9

2

Question 10

Sub shell definition

Answer 10

A specific energy level within an electron shell

Question 11

Order of increasing energy subshell

Answer 11

S, p, d, f

Question 12

Pauli exclusion principle

Answer 12

States only a maximum of two electrons may be found in a given atomic orbital and if an orbital is filled, electrons will have opposite spin

Question 13

Aufbau principle

Answer 13

States subshells are filled in order form lowest energy to highest energy and a lower energy subshell will be completely filled before electrons move into a higher energy shell

Question 14

Hunds rule

Answer 14

States electrons in a partially filled subshell will arrange themselves so as to form the maximum number of half filled orbitals

Question 15

Difference between atom in its ground state and atom in excited state

Answer 15

Atom in ground state has all electrons in lowest possible subshells whereas an atom in an excited state temporary has one or more electrons in higher energy subshell than the lowest possible

Question 16

Actual configuration copper

Answer 16

1s2 2s2 2p6 3s2 3p6 4s1 3d10

Question 17

Actual configuration chromium

Answer 17

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Question 18

Trends in atomic radius-> things need to talk about

Answer 18

-core charge
- number of occupied energy levels

Question 19

Core charge

Answer 19

Measure of the net attractive force felt by valence shell electrons towards nucleus

Question 20

Core charge calculation

Answer 20

Number of protons- number of electrons in inner shells

Question 21

Trends in atomic radii down a group

Answer 21

Atomic radius increases

Question 22

Why does atomic radius increase down a group

Answer 22

• number of occupied energy levels increases
• core charge remains constant

Question 23

Sodium and potassium which is bigger

Answer 23

Both in g1- both have constant core charge of 1+
Sodium has 3 occupied shells whereas potassium has 4 occupied shells t/f potassium is larger

Question 24

Trends in atomic radii across a period

Answer 24

Atomic radius decreases

Question 25

Why does atomic radius decrease across a period

Answer 25

Number of occupied energy levels remains constant Core charge increases-> valence electrons more strongly attracted to nucleus

Question 26

Electronegativity definition

Answer 26

Strength with which atoms of an element attract electrons when chemically combined with another element

Question 27

What does a higher electronegativity mean

Answer 27

Atoms are more able to pull shared electrons in covalent bond towards their nucleus

Question 28

Electronegativity will be higher when

Answer 28

Atomic radius is low Core charge is high

Question 29

Trend in electronegativity down a group

Answer 29

Electronegativity decreases

Question 30

Why does electronegativity decrease down a group

Answer 30

Number of occupied energy shells increase-> atomic radius increases Nuclear charge and electron shielding increases Overall means outermost electron is further from the nucleus and there are more electrons between an atoms nucleus and outermost electron meaning outermost electrins are less attracted towards nucleus

Question 31

Trend in electronegativity across a period

Answer 31

Electronegativity increases

Question 32

Why does electronegativity increase across a period

Answer 32

Number of occupied energy shells= constant Core charge increases + Atomic radius decreases Nuclear charge increases + electron shielding= constant T/f due to inc. core charge, valence electrons more strongly attracted to nucleus t/f inc. electronegativity

Question 33

Ionisation energy

Answer 33

Amount of energy required to remove an electron from each mole of gaseous atoms

Question 34

Factors that affect ionisation energy

Answer 34

As electrons are neg. Charged and protons= positively charged, there is an attraction between electrons and protons. Greater the pull of the nucleus, harder it is to pull an electron away from an atom

Question 35

As you move down a group, what happens to first ionisation energy and why

Answer 35

First ionisation energy decreases B/c - number of occupied energy shells increases so atomic radius increases and t/f nuclear attractions decrease - electron shielding increases and core charge= constant T/f less energy required to remove an electron

Question 36

As you move across a period, what happens to first ionisation energy and why

Answer 36

Increases b/c Number of occupied energy shells= constant and atomic radius decreases t/f outermost electrons closer to nucleus Core charge inc.-> outermost electrons more strongly attracted to nucleus T/f more energy required to remove and electron

Question 37

Electrons with low ionisation energies generally have low/high electronegativity and why

Answer 37

Low electronegativity b/c nuclei not exert strong attractive force on e

Question 38

Electrons with high ionisation energies have low/high electronegativity and why

Answer 38

High electronegativity b.c of strong pull exerted by on electrons

Question 39

Reactivity of metals: trends across a period

Answer 39

-core charge increases as we move across a period - electron shielding remains constant T/f increase energy required to remove an electron (inc. first ionisation energy) T/f reactivity of metals decreases across a period

Question 40

Reactivity of metals down a group

Answer 40

Core charge stays the same Number of energy levels and electron shielding increases-> decreases energy required to remove an electron T/f Dec. reactivity of metals

Question 41

Reactivity of non metals

Answer 41

Non metals with greatest attractive force will be most reactive Reactivity increases across a period Decreases down a group

Question 42

RAM calculation

Answer 42

(Relative abundance x relative isotopic mass 1) + (relative abundance x relative isotopic mass 2)/100