Structure and Bonding

Question 1

How many electrons can an s subshell hold?

Answer 1

2

Question 2

How many electrons can a p subshell hold?

Answer 2

6

Question 3

How many electrons can a d subshell hold?

Answer 3

10

Question 4

How many electrons can a f subshell hold?

Answer 4

14

Question 5

What is Aufbau principle?

Answer 5

Electrons always inhabit the lowest energy orbitals available

Question 6

Electrons repel each other so what holds them together and why?

Answer 6

Spin creates magnetism (moving charge)

Opposite spin creates opposite magnetic fields

Question 7

What is does electronegativity mean?

Answer 7

How attractive a nucleus is to electrons

Question 8

What are the properties that affect electronegativity?

Answer 8

Larger charge=more attractive

Charge density, more neutrons “dilute” positive charge =lower attractive

Inner electrons shield outer electrons reduces attraction

Distance, the further away, the weaker the attraction

Question 9

What is the most electronegativity element

Answer 9

Fluorine

Question 10

Why does ionic bonding occur?

Answer 10

Because the non-lethal has higher electronegativity so it steals electrons from the metal

Question 11

Why does convent bonds occur?

Answer 11

Similar electronegativity so they share electrons instead of stealing

Question 12

Why does metallic bonding occur?

Answer 12

Same electronegativity so they share electrons between the positive nucleuses
Delocialised electrons

Question 13

What happens to electronegativity across periods?

Answer 13

Adds protons so it increases

Question 14

What happens to electronegativity down groups?

Answer 14

More distance and more shielding so decreasing electronegativity

Question 15

What is stoichiometry?

Answer 15

The ratios of reactants

Question 16

What is promotion and why is it important?

Answer 16

Promotion is when electrons from 2s^2 move to 2p orbit
Promotion explains how carbon bond makes colavent bonds as it means a sub shell is freed up for an electron to bond

A mixture of s, p electrons forming a bond

Question 17

Ionic electron clouds look like

Answer 17

Cloud is more around the highly electronegative atom because more attractive to electrons

One side is denuded of electrons

Question 18

Colavent electron clouds look like

Answer 18

Even spread as similar electronegativities

Question 19

What are the 3 types of Van der Waals forces

Answer 19

Hydrogen bonding

London dispersion forces (temporary dipoles)

Permanent dipoles

Question 20

What are Van Der Waals forces

Answer 20

Weak attractive forces between molecules

Question 21

What is a tetrahedron and what angle between pairs?

Answer 21

The shape a molecule forms with one central atom and 4 bonded atoms

109.47°

Question 22

How do London dispersion forces work?

Answer 22

Electrons repel each other to create temporary positive charge in the charge cloud
The charged bits are then attracted to each other

Question 23

What is the order of strength of Van Der Waals forces?

Answer 23

Hydrogen
Permanent dipoles
London dispersion forces

Question 24

How do you work out moles?

Answer 24

Moles = Mr/Mass

Question 25

What order do the orbital go in?

Answer 25

S, p, d, f

Question 26

How do you calculate molar mass?

Answer 26

Mass/moles

Question 27

How do you calculate concentration?

Answer 27

Moles/volume

Question 28

What are the uses for magnesium oxide?

Answer 28

``` Fertilizer Mineral supplement Ice control Dust control Coagulant for making food Spa treatment ```

Question 29

Explain why copper is ductile?

Answer 29

Metallic bonding means a regular pattern This means atoms can slip past each other easily So metals can be drawn into wires without breaking

Question 30

Balance equation for the reaction of silicon and oxygen

Answer 30

Si + O^2 –⟩ SiO^2

Question 31

What is the force called between ions?

Answer 31

Electrostatic force

Question 32

What is the formulae of hydroxide?

Answer 32

OH-

Question 33

What is the formulae of carbonate

Answer 33

CO3²- small low 3

Question 34

What is the formulae of sulphate

Answer 34

SO4²- small low 4 small high 2

Question 35

What is the formulae of nitrate

Answer 35

NO3- small low 3

Question 36

What is the formulae of ammonium

Answer 36

NH4+ small low 4

Question 37

How do you work out molarity?

Answer 37

Molarity= moles/ litres of solution

Question 38

What is Aufbau principle?

Answer 38

Electrons will fill the orbital with the lowest available energy state

Question 39

What intermolecular forces do noble gases have?

Answer 39

London dispersion forces

Question 40

How do you work out percentage yield with moles?

Answer 40

Actual number of moles/expected number of moles *100

Question 41

What is an element?

Answer 41

A substance made from one type of atom

Question 42

What is a quantum?

Answer 42

A quantum is how much energy an electron needs to move to the next energy level Losing energy is dropping a level Gaining energy is moving up a level

Question 43

What's important to remember when drawing calcium electron configuration which has 20 electrons?

Answer 43

4s fills in before 3d

Question 44

What is the structure of ionic compounds?

Answer 44

Lattice giant structure usually regular pattern

Question 45

What does the strength of an ionic bond depend on?

Answer 45

More charge means more electrostatic forces Smaller ionic radius electrons are closer to the nucleus

Question 46

What is a dative bond?

Answer 46

Where the electrons come from the same atom, Colavent bond

Question 47

What affects the strength of covalent bonds

Answer 47

Shorter covalent bonds on a stronger closer to the nucleus Multiple bonds are stronger

Question 48

Why are metals good conductors of heat?

Answer 48

At higher temperatures metal atoms vibrate more. Bypass this vibration energy (kinetic/heat) to their neighbours Free electrons carry energy through the metals

Question 49

Why are metals good conductors of electricity?

Answer 49

Electrons are delocalized and negatively charged Free electrons can move through the metal and current is the flow of charge

Question 50

Why does the melting point decrease as we go down metals groups?

Answer 50

The atoms of bigger as they have more shells The distance between the nucleus and the delocalized electrons are bigger The forces holding the structure together are weaker

Question 51

What are inter-molecular forces and their name?

Answer 51

The forces between molecules Van de Waals forces

Question 52

Why are elements put into groups?

Answer 52

Put into groups of similar properties

Question 53

How many elements is there?

Answer 53

92

Question 54

What is electron affinity and what is it measured in?

Answer 54

How likely a neutral atom is to gain an electron Measured in the energy released Kj/mol