Lecture one

Question 1

What are the 3 key properties of elements

Answer 1

atomic radius
1st ionisation energy
electronegativity

Question 2

what is electronegativity

Answer 2

relative attraction an element has for a shared pair of electrons

Question 3

How does atomic radius vary across the periodic table

Answer 3

decreases across
increases down a group

Question 4

How does 1st ionisation energy vary in the periodic table

Answer 4

increases across
decreases down a group

Question 5

how does electronegativity vary within the periodic table

Answer 5

increases across
decreases down

Question 6

define a metal

Answer 6

are elements that lose electrons to form cations

Question 7

what’s a characteristic of a metal

Answer 7

low electronegativities and ionization energies

Question 8

give 5 properties of metals

Answer 8

shiny
high melting solids not mercury
conduct heat and electricity
strong and malleable
high density

Question 9

define non-metal

Answer 9

elements that gain electrons to form anions

Question 10

What’s a characteristic of a non metal

Answer 10

have high electronegativities and ionisation energies

Question 11

what does metals and non-metals form

Answer 11

ionic compounds

Question 12

give 4 properties of non-metals

Answer 12

dull
powdered solids, liquid or gases
does not conduct heat and electricity
low density

Question 13

What else are metals

Answer 13

Lewis acids and accepts electrons

Question 14

what’s the electrons lost (n) usually predicted from electron configuration

Answer 14

oxidation number

Question 15

What else are non-metals

Answer 15

Lewis base and donates electrons

Question 16

what does a Lewis acid and a Lewis base produce

Answer 16

coordination compound

Question 17

What bonding is in Lewis acid-base complexes

Answer 17

coordinate or dative

Question 18

where does this bonding come from

Answer 18

the Lewis base

Question 19

Properties of s-block metals

Answer 19

lose 1 or 2 electrons to form metals with octet configuration
fixed oxidation states
react most violently with water

Question 20

What bonding is in s-block

Answer 20

highly ionic

Question 21

What does oxidation state equate to

Answer 21

Charge of the metal ion

Question 22

Whys is the bonding in the s-block highly ionic

Answer 22

Due to low electronegativities so electrons are lost easily as they are repelled to remain as highly charged cations

Question 23

is OS easy to predict in s-block

Answer 23

Yes

Question 24

Give two reasons why predicting the Oxidation states of the p-block is more complicated

Answer 24

1 not always in octet configuration
2 bonding is more covalent due to higher electronegativities

Question 25

True or false - p-block highly poisonous

Answer 25

true

Question 26

Define inert pair effect

Answer 26

heavier metals tend to keep two valence electrons

Question 27

what happens when you go down group 3

Answer 27

the energy between 3s and 3p increases so cannot form covalent bonds so they're kept as lone pairs or lose the one valence electron

Question 28

What happens to Boron in p-block

Answer 28

Boron valence electrons 3s2 3p1 have a low energy so combine and hybridise to form 3 covalent bonds

Question 29

Define formal oxidation state

Answer 29

the + or – charge an element would have in a compound, if that compound was ionic

Question 30

give 3 properties of d-block metals

Answer 30

1 highly coloured ions 2 different oxidation states 3 form complexes with different geometries

Question 31

How can we work out the maximum known oxidation state

Answer 31

By adding the valence electrons up

Question 32

true or false - this is always seen in the first row

Answer 32

false

Question 33

Why for later transition metals does the maximum known oxidation states decrease

Answer 33

Because electronegativity increases

Question 34

Define ligand

Answer 34

species that binds to a metal and provides both bonding electrons

Question 35

What does a complex ion consist of

Answer 35

oxidation state and a ligand

Question 36

What is everything inside the bracket directly bound to

Answer 36

ligand / lewis base

Question 37

Whats outside the square bracket

Answer 37

oxidation state

Question 38

Examples of neutral ligands

Answer 38

amines, alcohols,ethers,water,phosphines and thioethers

Question 39

what are -1 ligands

Answer 39

halides, conjugate bases of neutral ligands

Question 40

examples of -1 ligands

Answer 40

F-, Cl-, OH-, NH2-

Question 41

examples of -2 and -3 ligands

Answer 41

oxo (-2) , sulfide(s2-), sulfate(SO42-) , nitride (N3-)

Question 42

Ligands that bind through one atom are called

Answer 42

monodentate

Question 43

Ligands that bind through two atoms are called

Answer 43

Bidentate

Question 44

Ligands that bind through three atoms are called

Answer 44

tridentate

Question 45

Define coordination number

Answer 45

the number of metal-ligand bonds in a complex

Question 46

define denticity

Answer 46

the number of atoms in a given ligand bound to a metal

Question 47

define chelating ligand

Answer 47

a ligand that binds to a metal using two or more atoms forming a chelate ring.

Question 48

Define donor atom

Answer 48

the atom of a ligand that bind to the metal

Question 49

define inner-coordination sphere

Answer 49

the ligands in a complex that bind directly to the metal

Question 50

define outer coordination sphere

Answer 50

the ligands that are a part of a complex, but that do not bind directly to the metal

Question 51

What are the steps of calculating oxidation states

Answer 51

take charge of the ligand calculate charge outside square brackets