Untitled Deck

Question 1

What is the relative charge and mass of a proton?

Answer 1

+1, mass = 1.

Question 2

What is the relative charge and mass of a neutron?

Answer 2

0, mass = 1.

Question 3

What is the relative charge and mass of an electron?

Answer 3

–1, mass ≈ 1/2000.

Question 4

Define isotopes.

Answer 4

Atoms of the same element with the same number of protons but different numbers of neutrons. they have the relative mass of one so this changes the mass number of the atom .

Question 5

Define relative atomic mass (Ar).

Answer 5

Weighted mean mass of an atom compared with 1/12 of carbon-12.

Question 6

Define relative molecular mass (Mr).

Answer 6

Weighted mean mass of a molecule compared with 1/12 of carbon-12.

Question 7

What is the equation for relative atomic mass from isotopes?

Answer 7

Ar = Σ(isotopic mass × abundance) / Σ(abundance).

Question 8

Define first ionisation energy.

Answer 8

Energy required to remove 1 mole of electrons from 1 mole of gaseous atoms.

Question 9

Why does first ionisation energy decrease down a group?

Answer 9

More shielding + larger atomic radius → weaker attraction between nucleus and outer electron.

Question 10

Why does first ionisation energy increase across a period?

Answer 10

More protons, same shielding → stronger nuclear attraction.

Question 11

State the general trend in successive ionisation energies.

Answer 11

They increase, with a big jump after all outer electrons are removed.

Question 12

What does a big jump in ionisation energy indicate?

Answer 12

The electron removed was from a new, inner shell which requres more energy due to its strong attcatction → shows group number.

Question 13

What is the electron configuration of oxygen (Z=8)?

Answer 13

1s² 2s² 2p⁴.

Question 14

State the order of orbital filling.

Answer 14

1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p.

Question 15

State Hund’s rule.

Answer 15

Electrons occupy orbitals singly before pairing.

Question 16

Which orbital fills first: 3d or 4s?

Answer 16

4s fills before 3d, but 4s electrons are lost first when ionising.

Question 17

Why does aluminium have a lower first ionisation energy than magnesium?

Answer 17

Outer electron in 3p orbital → higher energy, easier to remove.

Question 18

Why does sulfur have a lower first ionisation energy than phosphorus?

Answer 18

sulfur has Paired electrons in 3p orbital which repel each other while phosphorus has unpaired electrons → easier to remove one.

Question 19

what is a nuclides

Answer 19

any atom of which the atomic number and the mass number are specified

Question 20

anion

Answer 20

negative ion

Question 21

cation

Answer 21

positive ion

Question 22

what is the relative formula mass of MgCl2

Answer 22

24.3+(35.5x2)=95.3

Question 23

what are the four types of subshells

Answer 23

s,p,d,f

Question 24

how many orbitals are in the d subshell

Answer 24

10 electrons

Question 25

how many orbitals are in the f subshell

Answer 25

14 electrons

Question 26

how are the orbitals filled according to the Aufbau principle

Answer 26

the lowest available energy level (closet to the nucleus ) is filled first

Question 27

what is the noble gas notation of helium

Answer 27

(HE) 2s 2p4

Question 28

what is the trend of ionising energy across a period

Answer 28

energy increase as theres a stronger attraction therefore more protons

Question 29

trend of ionising energy down the group

Answer 29

energy decrease as electrons are further away and more shielding

Question 30

what are the 4 key factors of ionising energy

Answer 30

-nuclear charge (protons) -distance from the nucleus -electron sheilding -electron subshells

Question 31

what is the factor of nuclear charge in ionising energy ?

Answer 31

more protons - stronger attraction between nucleus + electrons - higher energy

Question 32

what is the factor of distance from nucleus in ionising energy

Answer 32

electrons further from the nucleus are less strongly attracted - lower ionising energy

Question 33

what is the factor of electron shielding in ionising energy

Answer 33

inner shells repel outer electrons reducing the pull of the nucleus - lower ionisation energy

Question 34

what is the factor of electron sub shell in ionising energy (stability)

Answer 34

half or fully filled are more stable - harder to remove electron - more energy

Question 35

why is ionising energy important

Answer 35

-shows how strong atoms hold together - reactivity -metals -low ionising

Question 36

formula with charge of hydroxide

Answer 36

OH-

Question 37

formula with charge of nitrate

Answer 37

NO3-

Question 38

formula with charge of sulfate

Answer 38

SO4-

Question 39

formula with charge of phosphate

Answer 39

PO3-

Question 40

write this in words : Tin(II) nitrate

Answer 40

Sn(NO3)2

Question 41

write this in words : calcium hydroxide

Answer 41

Ca(OH)2

Question 42

how to remember the diatomic molecules

Answer 42

Have - hydrogen No - nitrogen fear - Fluorine of - oxygen ice - iodine cold - chlorine beer- bromine

Question 43

metallic bonding

Answer 43

metal+metal and results in giant metallic lattice - Fe

Question 44

ionic bonding

Answer 44

metal + non-mental results in giant ionic lattice - NaBr

Question 45

covalent bonding

Answer 45

non metals + non metals resulting to simple molecules or giant covalent lattice - BF3

Question 46

what is the metallic bond

Answer 46

the strong electrostatic attraction between cations and delocalised electrons

Question 47

why are metals malleable

Answer 47

postive ions can slide past each other whilst retaining strong forces between particles in new arrangement

Question 48

W?hat holds metals together in metallic bonding?

Answer 48

Strong electrostatic attraction between positive metal ions and delocalised electrons.

Question 49

Why do metals conduct electricity?

Answer 49

Delocalised electrons are free to move and carry charge.

Question 50

Why do metals have high melting points?

Answer 50

Strong metallic bonds require lots of energy to break.

Question 51

What is ionic bonding?

Answer 51

Electrostatic attraction between oppositely charged ions (metal cation + non-metal anion).

Question 52

What is a giant ionic lattice?

Answer 52

A 3D repeating structure of positive and negative ions held together by strong ionic bonds.

Question 53

Why do ionic compounds have high melting points?

Answer 53

Strong ionic bonds between ions require lots of energy to break.

Question 54

Why do ionic compounds conduct electricity when molten or dissolved?

Answer 54

Ions are free to move and carry charge.

Question 55

Why don’t solid ionic compounds conduct electricity?

Answer 55

Ions are fixed in the lattice and cannot move.

Question 56

What is covalent bonding?

Answer 56

A shared pair of electrons between two non-metal atoms.

Question 57

What is a giant covalent structure?

Answer 57

A 3D network of atoms joined by strong covalent bonds (e.g. diamond, graphite, SiO₂).

Question 58

Why does diamond have a very high melting point?

Answer 58

Each carbon makes 4 strong covalent bonds → giant 3D network.

Question 59

Why does graphite conduct electricity?

Answer 59

Delocalised electrons move between layers.

Question 60

What is dative covalent bonding (coordinate bonding)?

Answer 60

A covalent bond where both electrons in the shared pair come from one atom.

Question 61

Example of a molecule with dative bonding?

Answer 61

Ammonium ion (NH₄⁺) — N donates a lone pair to H⁺.

Question 62

Shape & bond angle of 2 bonding pairs, 0 lone pairs?

Answer 62

Linear, 180° ## Footnote (e.g. CO₂)

Question 63

Shape & bond angle of 3 bonding pairs, 0 lone pairs?

Answer 63

Trigonal planar, 120° ## Footnote (e.g. BF₃)

Question 64

Shape & bond angle of 2 bonding pairs, 1 lone pair?

Answer 64

Bent, ~118° ## Footnote (e.g. SO₂)

Question 65

Shape & bond angle of 4 bonding pairs, 0 lone pairs?

Answer 65

Tetrahedral, 109.5° ## Footnote (e.g. CH₄)

Question 66

Shape & bond angle of 3 bonding pairs, 1 lone pair?

Answer 66

Trigonal pyramidal, ~107° ## Footnote (e.g. NH₃)

Question 67

Shape & bond angle of 2 bonding pairs, 2 lone pairs?

Answer 67

Bent, ~104.5° ## Footnote (e.g. H₂O)

Question 68

Shape & bond angles of 5 bonding pairs, 0 lone pairs?

Answer 68

Trigonal bipyramidal, 120° (equatorial), 90° (axial) ## Footnote (e.g. PCl₅)

Question 69

Shape & bond angle of 6 bonding pairs, 0 lone pairs?

Answer 69

Octahedral, 90° ## Footnote (e.g. SF₆)

Question 70

Define electronegativity.

Answer 70

The ability of an atom to attract the bonding electrons in a covalent bond.

Question 71

Which element is the most electronegative?

Answer 71

Nuclear charge (more protons → higher EN) nuclear charge (more protons → higher EN) Shielding (less shielding → higher EN).

Question 72

What is the trend in electronegativity across a period?

Answer 72

Increases — more protons, same shielding, increased nuclear charge.

Question 73

What is the trend in electronegativity down a group?

Answer 73

Decreases — more shielding, more inner shells , weaker nuclear attraction.

Question 74

What makes a covalent bond polar

Answer 74

A separation of charge within a bond, with δ+ and δ– ends

Question 75

Give an example of a polar molecule.

Answer 75

HCl — electrons pulled towards Cl (δ–), leaving H (δ+).

Question 76

What type of intermolecular forces does electronegativity explain?

Answer 76

Permanent dipole–dipole interactions and hydrogen bonding

Question 77

What makes a covalent bond polar?

Answer 77

A difference in electronegativity between the two atoms.

Question 78

When is a molecule polar overall?

Answer 78

When dipoles do not cancel due to lack of symmetry (e.g. H₂O).

Question 79

What are the three types of intermolecular forces?

Answer 79

temporary dipole -dipole , permanent dipole–dipole interactions, hydrogen bonding.