2.2

Question 1

what is an orbital

Answer 1

a region around the nucleus that cab hold up to 2 electrons, each with opposite spin

Question 2

what are the 4 types of orbitals?

Answer 2

s,p,d,f

Question 3

shape of s orbital?

Answer 3

spherical

Question 4

shape of p orbital?

Answer 4

dumbbell

Question 5

how many orbitals fit into s sub shells

Answer 5

1

Question 6

how many orbitals fit into p sub shells

Answer 6

3

Question 7

how many orbitals fir into d sub shells

Answer 7

5

Question 8

which orbital is filled and empties before 3d

Answer 8

4s

Question 9

what are the 3 rules for writing out electrical configuration?

Answer 9

• lowest energy orbital is filled first
• for orbitals with the same energy, electrons occupy orbitals singly with the same spin before pairing
• no orbital holds more than 2 electrons

Question 10

what is ionic bonding?

Answer 10

electrostatic attraction between positive and negative ions. occurs between a metal and non-metal. electrons are transferred from the metal to the non-metal to non -metal so both elements achieve a full outer shell.

Question 11

how are giant ionic lattices formed?

Answer 11

when the electrons are transferred, it creates charged particles called ions. oppositely charged ions attract each other through electrostatic forces to form giant ionic lattices.

Question 12

how can the attraction of an ion change?

Answer 12

• ions with a greater charge will have a greater attraction to other ions resulting in stronger forces of attraction therefore stronger ionic bonds
• larger ions that have a greater ionic radius will have a weaker attraction to the oppositely charged ion as the forces will have to act over a greater distance

Question 13

what are the physical properties of ionic bonding?

Answer 13

• substances with ionic crystal structures have a high melting point and boiling point because the electrostatic forces holding the ionic lattice together are strong - require lots of energy to overcome
• when molten/aqueous, ionic substances can conduct electricity as the ions separate and are no longer held in lattices therefore they are free to move and carry a flow of charge
• in a solid state, ions are in fixed positions with no mobile charge carrier so cannot conduct electricity
• ionic substances are often brittle metals. when the layers of alternating chargers are distorted, like charges repel, breaking there lattice into fragments

Question 14

what is covalent bonding?

Answer 14

• the strong electrostatic attraction ion between a shared pair of electrons and the nuclei of the bonded atom
• between 2 nonmetals, electrons are shared between two outer shells in order to achieve a full outer shell. multiple electron pairs can be shared to produce multiple covalent bonds

Question 15

how does the length of a covalent bond relate to its strength?

Answer 15

shorter bonds tent top be stronger (atoms are held closer together so force of attraction are greater, requiring more energy to overcome) double/triple bonds = stronger than single bond

Question 16

what is used as a measure of covalent bond strength?

Answer 16

average bond enthalpy

Question 17

dative covalent bonds

Answer 17

form when both of the electrons in the shared pair are supplied by a single atom. indicated using an arrow from the lone electron pair

Question 18

what is the shape of molecules determined by

Answer 18

the number of electron pairs around the central atom and repulsion between them
- each electron pair naturally repels each other so that the largest possible bond angle exists

Question 19

VESPR theory

Answer 19

BP-BP<BP-LP<LP-LP

Question 20

define electronegative

Answer 20

the ability of an atom ton attract the bonding electrons in a covalent bond towards itself

Question 21

how does electronegativity vary along a period?

Answer 21

increases, atomic radius decreases and charge density increases

Question 22

how does electronegativity vary down a group?

Answer 22

decreases, shielding increases and atomic radius so charge density decreases

Question 23

what scale is used to test electronegativity

Answer 23

pauling scale

Question 24

permanent dipoles

Answer 24

if the 2 two atoms that are bonded have different electronegativities, a polar bond forms. the more electronegative atom draws more of the negative charge towards itself and away from other atom, producing a slightly + and - region

Question 25

what do polar molecules require

Answer 25

polar bonds with dipoles that do not cancel each other out

Question 26

when do induced dipoles form

Answer 26

when the electron orbitals around a molecule are influenced by the distribution of electrons on another particle

Question 27

what is the strongest type of IMF

Answer 27

hydrogen bonding

Question 28

which elements does hydrogen bonding act between

Answer 28

hydrogen
Nitrogen
Oxygen
Fluorine