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IB Chemistry HL > 3. Periodicity > Flashcards

3. Periodicity Flashcards

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1
Q

What are the factors that affect atomic radius? [2]

A

Nuclear charge

Shielding effect by inner electrons

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2
Q

What is the effective nuclear charge?

A

The difference between nuclear charge and shielding effect

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3
Q

What is the periodic trends in atomic radius?

A

Increase down the group

Decrease across a period

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4
Q

What is the general trend for ionic radius?

A

Radii of cations are smaller than parent atom

Radii of anions are bigger than parent atom

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5
Q

What is the periodic trend for ionic radius?

A

Cation:
Decrease down a period, increase down a group

Anion:
Decrease down a period, increase down a group

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6
Q

What is the defi of 1st ionisation energy?

A

The minimum energy required in removing one mole of valence electrons from one mole of gaseous atoms to form 1 mole of singly positively-charged gaseous ion

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7
Q

Periodic trends for 1st ionisation energy

A

Increases across a period

Decreases down a group

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8
Q

What are the factors affecting ionisation energy across a period and down a group?

A

Period: Effective nuclear charge
Group: Atomic radii

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9
Q

What are the 2 exceptions in 1st ionisation energy trend? Explain.

A

Between group 2&13 (extra sub-level)

Between group 15&16 (how the electrons are arranged in the orbital)

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10
Q

What are the top 4 electronegative elements?

A

NOF Cl

Oxygen, nitrogen, fluorine, chlorine

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11
Q

Defi of electronegativity

A

The relative attraction that an atom has for the shared pair of electrons in a covalent bond

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12
Q

What is the periodic trend of electronegativity? Explain.

A

Increase across a period
Decrease down a group

As electrostatic attraction between bonding electrons and nuclei increases, electronegativity will increase

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13
Q

What is the first electron affinity?

A

The enthalpy change when one mole of gaseous atoms acquires one mole of electrons to form one mole of singly negatively charged gaseous ions

S(g) + e- –> S- (g)

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14
Q

Is first electron affinity exo or endothermic?

A

Exothermic for most elements

Energy released when nucleus attracts electron in outer shell (like bond forming)

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15
Q

What is the periodic trend for first electron affinity?

A

Increases across a period

Decreases down a group

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16
Q

What is the exception for first electron affinity? Why?

A

Nitrogen
Addition of an extra electron –> Energy needed to overcome the inter-electronic repulsion between the paired electrons –> Less exothermic

17
Q

How to explain fluorine and oxygen for electron affinity?

A

Energy released when nucleus attracts an electron is far greater than energy needed to overcome inter-electronic repulsion

18
Q

Defi of second electron affinity?

A

The enthalpy change when one mole of singly negatively-charged gaseous ions acquires one mole of electrons to form one mole of doubly negatively-charged gaseous ions

19
Q

What is the enthalpy change for second electron affinity? Why?

A

Endothermic
Always positive enthalpy, meaning we need energy
To overcome repulsion between 2 negatively-charged species (electron & anion)

20
Q

Between period 2 & 3, what are the giant covalent structures (elements)

A

Boron, Silicon, Carbon (can also form C60)

21
Q

What are the simple molecules between periods 2 & 3 (elements only)?

A

C60, N2, O2, F2, P4, S8, Cl2

22
Q

What is the periodic trend for melting point for metals?

What is one exception to take note of for period 3?

A

Increases across a period

Silicon is higher than Al due to its giant covalent structure

23
Q

Why does metallic bond strength increase across the period?

A
  1. Decrease in metallic radius
  2. Increase in no. of electrons donated per atom to the mobile sea of electrons

==> Increase in charge density

24
Q

What is the periodic trend for non-metals?

A

Decreases across a period
Increases down a group

Due to LDF increasing down a group due to larger electron clouds

25
Q

What is the trend of melting points down group 1?

A

Decreases down the group
Decrease in strength of metallic bond
Decrease in EFOA between cations & sea of delocalised electrons

26
Q

What is the trend of melting points down group 17?

A

Increases down the group

Increase in LDF

27
Q

What is the trend of reactivity of group 1 & 17?

A

Group 1: Increases down the group

Group 17: Decreases down the group

28
Q

Alkali metal (group 1 metals ) + H2O –> ?

A

Metal hydroxide + hydrogen gas

29
Q

Match: Group 1, Group 17, reducing agent, oxidising agent

A

Group 1 - reducing agent

Group 17 - oxidising agent

30
Q

What are the most reactive non-metals and metals?

A

Non-metal: Fluorine

Metal: Francium

31
Q

How to determine presence of halide ions?

A 
Add silver nitrate solution
Silver ions will react with halide ions to form precipitate
AgCl: White
AgBr: Cream
AgI: Yellow
32
Q

What is a displacement reaction?

A

A reaction where a more reactive halogen replaces another halide ion in a compound

33
Q

Name all period 3 oxides

A 
Na2O
MgO
Al2O3
SiO2
P4O6/P4O10
S02/SO3
34
Q

Name the type of structure of period 3 oxides

A

Na/Mg - giant ionic lattice
Al - giant ionic lattice with partial covalent character
Si - giant covalent structure
P/S - simple molecular structure

35
Q

What are the reactions of period 3 oxides with water?

A 
Na --> NaOH
Mg --> Mg(OH)2 (sparingly soluble)
Al/Si: No reaction
P --> H3PO4/H3PO3
S --> H2SO3/H2SO4
36
Q

What does an amphoteric oxide do?

A

Reacts with both acids and strong bases

37
Q

What is the equation for oxides of phosphorous with water?

A

P4O6 (s) + 6H2O (l) –> 4H3PO3 (aq)

P4O10 (s) + 6H2O (l) –> 4H3PO4 (aq)

38
Q

What is the equation of oxides of sulfur with water?

A

SO2 (g) + H2O (l) –> H2SO3 (aq)

SO3 (l) + H2O (l) –> H2SO4 (aq)

IB Chemistry HL (7 decks)

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