Week 1 Matter

Question 1

What is a Quantum?

Answer 1

The smallest amount of energy that ca be emitted/absorbed as electroradition.

Question 2

What is Planck’s constant?

Answer 2

6.626 X 10^-34 (Joules seconds)

Question 3

What is Planck’s theory?

Answer 3

Matter is allowed to emit/absorb energy only in whole number multiples.

Question 4

What are the 2 rules of Bohr’s model.

Answer 4

1. Electrons exist only in certain discrete energy levels, which are described by quantum numbers.
2. Energy is involved in moving an electron from one level to another.

Question 5

What is the orbitals probability density?

Answer 5

The orbitals probability density describes a specific distribution of electron density in space.

Question 6

What is the principal quantum number (n)

Answer 6

This number describes the size of the orbital, with 1 being the smallest. An increase in (n) means the orbital electron is less tightly bound to the nucleus.

Question 7

What is the angular momentum quantum number (i)

Answer 7

Defines the shape of the orbital, with values from 0 to n -1. E.G n=3, i=0,1,2.

Question 8

What is the magnetic quantum number (m)

Answer 8

Describes the orientation of the orbital in space via integral values between -1,0,1

Question 9

What is the electron shell

Answer 9

A collection of orbitals with the same value of (n) E.G n=3 is the third shell

Question 10

What is a subshell?

Answer 10

A set of orbitals that have the same (n) and (i) values.

Question 11

What are degenerate orbitals?

Answer 11

Orbitals wit the same energy.

Question 12

What is the Pauli exclusion principle?

Answer 12

No two electrons can have he same set of four quantum numbers (n,i,Mi, and Ms) in the same atom.

Question 13

Wha is the electron configuration?

Answer 13

The way in which the electrons are distributed among the various orbitals of an atom.

Question 14

What is the Aufbau principle?

Answer 14

Oribitals are filled in order of increasing energy, with no more than 2 electrons per orbital.

Question 15

What is hund’s rule?

Answer 15

For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximised.

Question 16

What are the Lanthanide elements?

Answer 16

The 14 elements corresponding to the filling of the 4f orbitals (rare earth elements)

Question 17

What are Actinide elements?

Answer 17

Elements in the final row of the periodic table that start to fill the 7s orbital (Radioactive).

Question 18

What is the Actual nuclear charge (Z)

Answer 18

The number of protons in the nucleus.

Question 19

What is the Effective nuclear charge?

Answer 19

The charge that valence electrons see.

Question 20

What is the Bonding atomic radius?

Answer 20

Half the distance between 2 identical atoms nuclei that are chemically bonded to each other.

Question 21

What is the Isoelectronic series?

Answer 21

A group of ions all containing the sae number of electrons.

Question 22

What is Ionisation energy?

Answer 22

The smallest amount of energy required to remove an electron from the ground state of the isolated gaseous atom or ion
(Lose of electron)

Question 23

What is Electron affinity?

Answer 23

The energy change that occurs when an electron is added to a gaseous atom or ion
(Gain of electron)

Question 24

What is an ionic bond?

Answer 24

Electrostatic forces between ions of opposite charge.

Question 25

What is a Covalent bond?

Answer 25

The sharing of electrons between 2 atoms.

Question 26

What is metallic bonds?

Answer 26

Each atom in a metal is bonded to several neighbouring atoms.

Question 27

What is the octet rule?

Answer 27

Atoms tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons.

Question 28

What are non-polar covalent bonds

Answer 28

Bonds where electrons are shared equally between two atoms

Question 29

What are polar covalent bonds

Answer 29

A bond where one of the atoms exert a greater attraction for the bonding electrons than the other atom

Question 30

What are resonance structures

Answer 30

A Lewis structure that has more than one correct way of displaying it

Question 31

What is a dipole moment

Answer 31

A quantitative measure of the amount of charge separation in the molecule

Question 32

What are addition reactions

Answer 32

The most characteristic reactions of alkenes and alkynes in which a reactant is added across the two carbon atoms that form the multiple bond

Question 33

What are Electrophiles

Answer 33

Molecules that accept a pair of electrons in a chemical reaction

Question 34

What are nucleophiles

Answer 34

Species that donates a pair of electrons in a chemical reaction

Question 35

What is a stereoselective reaction?

Answer 35

A reaction in which the product has one particular geometry in preference over another

Question 36

What does a Bold wedge indicate?`

Answer 36

Indicates that the direction of the bond is extending towards the viewer off the plane of the paper

Question 37

What does a dashed wedge indicate?

Answer 37

Indicates the direction of the bond is directed into the paper away from the viewer

Question 38

What is a Chiral

Answer 38

All molecules that contain a single carbon atom bearing four different groups

Question 39

What is a Enantiomer?

Answer 39

Two molecules that are non-superimposable mirror images | Always have a chiral centre

Question 40

What is a Achiral

Answer 40

Molecules that are superimposable. | Identified by their phone of symmetry

Question 41

What is a Dextrorotatory

Answer 41

An Isomer that rotates plane-polarised light to the right (+)

Question 42

What is a Levorotatory?

Answer 42

An enantiomer that rotates plane-polarised light to the left (-)

Question 43

What is optically active

Answer 43

Chiral molecules that effect plane-polarised light

Question 44

What is Enantiomerically pure

Answer 44

Containing a single enantiromer

Question 45

What is a Racemic mixture?

Answer 45

A mixture with an equal amount of both enantiomers

Question 46

What is a absolute configuration

Answer 46

The exact three-dimensional structure

Question 47

What is a Pi bond?

Answer 47

A covalent bond in which the overlap regions lie above and below the internucler axis

Question 48

What is Beer-lambert’s law

Answer 48

Relates to the amount of light being absorbed to the concentration of the substance absorbing the light.

Question 49

What is dispersion force

Answer 49

Instantaneous dipole attractive force on the adjacent atom

Question 50

What is dipole-dipole force

Answer 50

A permanent dipole moment in polar molecules

Question 51

What is ion-dipole force

Answer 51

Forces between an ion and a polar molecule

Question 52

What is a solution

Answer 52

When one substance disperses uniformly throughout another.

Question 53

What is a saturated solution

Answer 53

A solution that is in equilibrium with undissolved solute

Question 54

What is a unsaturated solution?

Answer 54

Less solute that is needed to form a saturated solution.

Question 55

How do you identify a Geometric isomers?

Answer 55

They have double bond between carbon

Question 56

How do you identify optical isomers?

Answer 56

Caron surrounded by 4 different chains (Chiral)