Inorganic

Question 1

What does Heisenberg’s uncertainty principle state?

Answer 1

The more accurate the data about a particles position the less accurately we know its momentum or vise versa

Question 2

What is electronegativity

Answer 2

The ability of an atom to attract an electron in a covalent bond

Question 3

Which is the only atom happy to be in a long chain of itself

Answer 3

Carbon all other atoms are very unstable in this form

Question 4

How do you draw Lewis structures

Answer 4

1. Add up the total number of valence electrons
2. Decide on the central atom
3. Join atoms together using single bonds
4. Keep adding the remaining pairs of electrons to form multiple bonds
5. Add the remaining electrons as lone pairs
6. Check the number of electrons in the surrounding atoms and add charges as necessary

Question 5

What are 2 exceptions for conventional Lewis structure rules

Answer 5

Some elements e.g. boron cannot achieve a full octet
Elements in the second or more rows can accommodate more than 8 electrons

Question 6

What is the mass in Kg of 1 amu

Answer 6

1 amu is the mass of a proton or neutron
1.6605 x 10E-27

Question 7

What are conformational isomers

Answer 7

These are isomers that can inter convert into one another by rotation around a single bond

Question 8

How are Newman projections drawn

Answer 8

1. The front C is shown as a dot
2. The back C is shown as a circle around the dot
3. The atoms bonded to the front C are shown drawn from that dot
4. The atoms bonded to the back C are shown drawn from the circle

Question 9

What does the wavefunction show

Answer 9

How likely he electron will be found in any given place at a given time

Question 10

What does the quantum number L represent

Answer 10

The orbital angular momentum quantum number and is a maximum of 1 value lower then n

Question 11

What is the chance of finding ell of the electrons in what is generally considered the radius of the atom

Answer 11

90%
Because the radius of an atom is set so that the chance of finding all electrons in the atom is 90%

Question 12

When does shrodingers equation fail and why

Answer 12

Shrodingers equation fails when more than 1 electron is present and this is because the energy of atoms depends on n and l quantum numbers rather then just n

Question 13

What do radial probability functions show

Answer 13

The area under a radial probability function graph shows the likelihood of finding one electron in a specific distance from the nucleus

Question 14

What happens if an electron penetrates the shielding of an energy level

Answer 14

It gains an increase in effective nuclear charge

Question 15

What is the equation for calculating effective nuclear charge

Answer 15

Z(eff) = Z (nuclear charge) - S (slaters rule)

Question 16

What are the rules for calculating slaters number used to measure effective nuclear charge

Answer 16

1. Orbitals are subdivided (1s) (2s, 2p) (3s, 3p) (3d) etc
2. No contribution to S from any brackets to the right of the selected electron
3. 0.35 is added to S for each electron in the same bracket other than the one being measured
4. The next lowest entire group adde 0.85 onto s for each electron
5. The next adds 1.00
6. Ignore rules 4 and 5 if the electron being considered is on an F or D orbital and instead add 1.00 for each electron lower thank it

Question 17

What are the possible spin values for electrons in an atom

Answer 17

+1/2 or -1/2
Each electron in an orbital must have a different spin

Question 18

When a new electron is added to a molecule where will it go (favourite option to least favourite option)

Answer 18

A new unoccupied available orbital in the same energy level
An occupied orbital in the same orbital spinning parallel to previous electrons
An orbital at a higher energy level

Question 19

Why does an increase in D and F electrons not increase the atomic radius as expected

Answer 19

D and F orbitals aren’t very good shields so can’t keep up with the increase in nuclear charge meaning the outer electrons are more strongly attracted to the nucleus then would be expected

Question 20

By what method do we determine the three dimensional shape of covalent molecules

Answer 20

VSEPR (valence shell electron pair repulsion)

Question 21

What are the 5 types of symmetric operations

Answer 21

1. Rotation - Cn
2. Reflection - sigma
3. Inversion - i
4. Rotation-reflection - Sn
5. Identity

Question 22

How do you determine what point group a molecule belongs too

Answer 22

First work out which of the 5 symmetric identities the molecule has then follow the flow chart provided to locate its specific point group

Question 23

What changes are made to VSEPR rules when determining double and triple bonds

Answer 23

One electron must be subtracted for double or 2 for triple bonds

Question 24

Which is more thermodynamically stable diamond or graphite

Answer 24

Graphite

Question 25

What does the acronym OIL RIG stand for

Answer 25

Oxidation is loss of electrons and reduction is gain of electrons