IQR 2

Question 1

Isotopes

Answer 1

Atoms of one element that differ by having different numbers of neutrons in their nuclei. The number of protons will remain the same. Isotopes are usually named by their mass.

Question 2

Atmoic number

Answer 2

NUmber of protons

Question 3

Mass number

Answer 3

The avarage mass of all isoptopes nucleus that include protons and neutrons.

Question 4

Relative atomic mass

Answer 4

The average mass of the atoms present in the naturally occurring element relative to the mass of an atom of the carbon-12 isotope, taken as 12 exactly.

Question 5

Relative molecular mass

Answer 5

Mass of a melecule of the compound relative to the mass of an atom.

Answer 6

i

Question 7

Another method of showing nuclear data. What does each character represent.

Answer 7

M is the chemical symbol
A is the mass number
z is the Atmoic number

Question 8

Electron configuration formula

Answer 8

2n^2

Question 9

The elctron cloud

Answer 9

Region around the nucleus where elctrons are most likely to be found. Electrons don’t move in fixed orbits but electron clouds with probability regions called orbitals.

Question 10

Nucleon

Answer 10

Sometimes used to describe either a proton or a neutron. The mass number is sometimes called the nucleon number.

Question 11

Relative abundance

Answer 11

Percentage of that isotope in the naturally occurring element.

Question 12

Electron configuration:

Answer 12

Determined by allocating electrons to energy levels

Question 13

Electron shells

Answer 13

Electron level, each cell is split into sub cells: SPDF

Question 14

Sub cells:

Answer 14

1.s
2.sp
3. spd
4.spdf
Every orbital has a maximum of two electrons
Each sub cell has different obital shape and number. Different orbitals have different energies.
Electrons fill the lowest available energy level that they can.
Electrons must fill orbital singularly before they buddy up.

Question 15

Orbital

Answer 15

Volume of space around the atom where one or 2 electrons randomly move.

Question 16

S orbital

Answer 16

Contains 1 orbital
2 electrons
shaped liek a sphere

Question 17

P orbital

Answer 17

3 orbitals
Dumbell shape arranged around axis at 90
6 electrons, 2 per orbital

Question 18

D orbital

Answer 18

5 orbitals,
10 electrons

Question 19

F orbital

Answer 19

7 orbitals
14 electrons

Question 20

Spin

Answer 20

No two electrons can be together with the same spin.

Question 21

Electron configuration example: Krypton

Answer 21

Question 22

Change in energy

Answer 22

Electrons can move between energy levels
Absorb Photons to move to higher energy level- excitation. Emit photons to move to lower energy level de-excitation.
The amount of energy absorbed/emitted by the electron must equal the different between the energy levels involved.

Question 23

Photon

Answer 23

A packet of light energy or electromagnetic radiation. Wavelengths determine the colour.

Question 24

Emission spectra

Answer 24

When an atom has electrons in higher levels that can move down to lower levels. THey emit phtons with energy based on the difference in electron energy levels. The photons of different colour (energy) will also have a different colour or wavelength.

Question 25

Absorption spectrum

Answer 25

Photos absorbed will have energies that match specific wavelengths. The spectrum of light we see will be missing specific colours.

Question 26

Stable elctron configurations

Answer 26

Noble gases: Completely filled energy levels Akali metals: Similar properties as they loose one electron Halogens: Similar properties as each gains one electron The driving force behind chemical reactivity is so that atoms can achieve the same electron configuration. Elements in the same group tend to gain or loose the same number of electrons transition elemts: 3-12 on table

Question 27

Valence electron and position ont he periodic table:

Answer 27

Number of valence electron to group is number 1,2, 13+ Group 14 can either be +4 or +2

Question 28

Principles

Answer 28

The lowest energy electrons are the ones closest to the nucleus.

Question 29

Bohr theory

Answer 29

Electron move around the nucleus in fixed orbits. When absord energy they moce to orbits of large radius then when emit energy they move to smaller radius. Incorporated Planck's quantum theory: Electrons could only have discrete energy levels Only could be used for simple spectra e.g Hydrogen.

Question 30

Schrodinger:

Answer 30

Treated the electron as a wave rather than a particle Applied mathematics to find location around nucleus (Schrodinger equation). Outcome: Finding the electron atoms anywhere in a spherical shape around the nucleus which contrasted bohrs fixed orbit idea Orbital was introduced when describing the space around the nucleus where your likely to find an electron. When applied to an atom with more than one elctron it leads to sublevels and orbitals. Equation used to interpret emission spectra with many electrons.

Question 31

Positron emission

Answer 31

Involves the emission of a positively charge particle, resulting from the changing of a proton into a neutron. (Happen when there is a surplus of protons) Chemical Symbol is

Question 32

Electron Capture

Answer 32

Opposite of an electron.

Question 33

Ethanol anion

Answer 33

[CH3COO]−

Question 34

Carbonate ion

Answer 34

Question 35

Hydrogen carbonate ion

Answer 35

Also called Bicarbonate

Question 36

Hydroxide Ion

Answer 36

Question 37

Nitrate Ion

Answer 37

Question 38

Phosphate Ion

Answer 38

Question 39

Sulfate Ion

Answer 39

Question 40

Unique about zinc and silver

Answer 40

Always a plus two.

Question 41

Flame test: Lithium

Answer 41

Red

Question 42

Flame test: Sodium

Answer 42

Yellow-Orange

Question 43

Flame test: Potassium

Answer 43

Pink

Question 44

Flame test: Calcium

Answer 44

Orange- red

Question 45

Flame test: Strontium

Answer 45

red

Question 46

Flame test: Barium

Answer 46

Pale green

Question 47

Flame test: Copper

Answer 47

Blue-green

Question 48

Limitations of the flame test

Answer 48

Only distinguishes between substances of a pure compound Some compounds have similar colours Colours are subjective Not all metal ions give colour under a flame.

Question 49

Aufbau's Principle

Answer 49

States that the lowest energy orbitals are always filled with electrons first. Energy levels start to overlap in energy. (Anomaly where 4s is before 3d)

Question 50

Pauli's Exclusion principle

Answer 50

An orbital only holds 2 electrons and the electrons in the same orbital have opposite spin. Because electrons spin, two can occupy one orbital.

Question 51

Hunds rule

Answer 51

Within a sublevel single electrons are placed one at a time in orbitals with spins of the same directions. Then will double up with electrons spinning the opposite direction

Question 52

Noble Gas electron configuration

Answer 52

When electrons configurations are written, noble gas notation is often used to represent filled shells. In noble gas notation, the symbol for a noble gas is written within square brackets in front of the spdf or orbital box notation representing additional electrons. The electron configuration can be abbreviated by indicating the innermost electron electrons with the symbol of the preceding noble gas.

Question 53

Exception to Aufbau rule

Answer 53

1. When orbitals are half-filled or filled by moving electrons

Question 54

Limitations of Bohr's model that lead to shrodinger's model

Answer 54

Bohr model could not interpret complex spectra. Didn't accept that the electron was not just a lump of matter but had wave properties. Schrodinger treated electrons as waves, that moved at high speeds throughout orbitals. Schrodinger created equation which used wave properties to calculate probability of finding an electron at a particular location.