Periodicity

Question 1 of 31

1

Describe the electronegativity and atomic radius trend across a period

Select one of the following:

The electronegativity decreases across a period
The atomic radius decreases across a period
The electronegativity increases across a period
The atomic radius decreases across a period
The electronegativity Increases across a period
The atomic radius increases across a period
The electronegativity decreases across a period
The atomic radius increases across a period

Explanation

Question 2 of 31

1

Melting point increases across a period

Select one of the following:

True
False

Explanation

Question 3 of 31

1

non-metals have a giant molecular structure meaning a lot of energy is required to break the bonds

Select one of the following:

True
False

Explanation

Question 4 of 31

1

Which two answers correctly describe electrical conductivity

Select one or more of the following:

electrical conductivity decreases down a group when they are conductable
electrical conductivity - made possible by ions or electrons that are not free to move
electrical conductivity across a period decreases overall
occurs in covalent bonds

Explanation

Question 5 of 31

1

Ionic radius decreases across the period until formation of the negative ions. Afterwards there is a sudden increase followed by a steady decrease to the end.

Is this true or false?

Select one of the following:

True
False

Explanation

Question 6 of 31

1

Why does sulphur have a higher melting point than phosphorous?

Select one or more of the following:

there are higher intermolecular forces between sulphur than phosphorous
there are lower intermolecular forces between sulphur than phosphorous

Explanation

Question 7 of 31

1

Which physical property increases down a group but decreases across a period

Select one of the following:

Ionic radius
Atomic radius
Electronegativity

Explanation

Question 8 of 31

1

Why are there no values for atomic radius for noble gases? (two answers)

Select one or more of the following:

The atomic radius doesn't affect their nuclear charge
Nuclei distance is difficult to measure
They do not generally bond to other atoms

Explanation

Question 9 of 31

1

Which is the correct order of decreasing radii for Cl, Cl+, Cl- ?

Select one of the following:

Cl, Cl-, Cl+
Cl+, Cl, Cl-
Cl-, Cl+, Cl
Cl-. Cl, Cl+

Explanation

Question 10 of 31

1

What are the chemical properties of Group 0 (Noble gases)?

Select one of the following:

odour, colourless, mono atomic, reactive
odourless, colourless, mono atomic, unreactive
odourless, colour, not mono atomic, unreactive
odour, colour, not mono atomic, reactive

Explanation

Question 11 of 31

1

What are the chemical properties of Group 1 (alkali metals)?

Select one of the following:

reactivity increases down group, 1 electron in outer shell, form ionic compounds, doesn't conduct electricity, very reactive, low density
reactivity decreases down group, 1 electron in outer shell, form ionic compounds, doesn't conduct electricity, very reactive, low density
reactivity increases down group, 1 electron in outer shell, form ionic compounds, conducts electricity, very reactive, low density
reactivity increases down group, 2 electron in outer shell, doesn't conduct electricity, very reactive, low density

Explanation

Question 12 of 31

1

Halogens reactivity increases down a group, they form ionic compounds with metals or covalently with non-metals, have 6 in the outer shell, diotomic

Select one of the following:

True
False

Explanation

Question 13 of 31

1

There is no displacement reaction in this equation because Iodine is weaker than Bromine

2KBr + I2 ----->

Select one of the following:

True
False

Explanation

Question 14 of 31

3

What are the characteristics of chlorides? (tick three)

Select one or more of the following:

Na, Mg - alkaline
Al - amphoteric
Si, P, S, Cl - alkaline
Si, P, S, Cl - acidic
Na, Mg - acidic

Explanation

Question 15 of 31

1

'Increasing charge density of the positive ion polarises the chloride ion as we move to the right hand side'. Is this true?

Select one of the following:

True
False

Explanation

Question 16 of 31

1

Here is a list describing and explaining the melting point trend across period 3. Which one is INCORRECT

Select one or more of the following:

Na -----> Al = steady increase as there is an increase in the availability of electrons in the metallic bonding
Si = massive increase since Si has a giant macromolecular structure
P = slight increase due to as have only van der Waals forces between molecules whereas the others have giant structures; P4 molecule
S = small increase as have only van der Waals forces between molecules whereas the others have giant structures; S8 molecule
P= large decrease as have only van der Waals forces between molecules whereas the others have giant structures; P4 molecule
Cl ---> Ar = decrease as chlorine is a much smaller molecule with weaker van der Waals forces; argon is just a single atom = very weak van der Waals forces

Explanation

Question 17 of 31

1

Which oxides are insoluble in water?

Select one or more of the following:

Na2O
MgO
Al2O3
SiO2
P4O10
(or P4O6)
SO3
(or SO2)
Cl2O7
Cl2O

Explanation

Question 18 of 31

1

Which oxides DO NOT react with HCl?

Select one or more of the following:

Na2O
SO3 (OR SO2)
Al2O3
P4O10 (OR P4O6)
SiO2
MgO
Cl2O7
Cl2O

Explanation

Question 19 of 31

1

Which ones react when NaOH is added?

Select one or more of the following:

Na2O
MgO
SiO2
H3PO4
SO2
HCl2O7
Al2O3

Explanation

Question 20 of 31

1

Oxides in period 3 are either Basic Oxide, Amphoteric Oxide or Acidic Oxide

Select one of the following:

True
False

Explanation

Question 21 of 31

3

Which ones have a good conductivity? (3 answers)

Select one or more of the following:

Na2O
Al2O7
SiO2
P4O10
MgO
Cl2O7

Explanation

Question 22 of 31

1

Melting point in period 3 oxides increases Na2O --> MgO and then decreases from MgO ---> Cl2O7

Select one of the following:

True
False

Explanation

Question 23 of 31

2

Which chlorides across period 3 dissolves in water?

Select one or more of the following:

NaCl
Al2Cl6
SiCl4
MgCl2
PCl3
PCl5
Cl2

Explanation

Question 24 of 31

1

Melting point increases across period 3 chlorides

Select one of the following:

True
False

Explanation

Question 25 of 31

1

NaCl and MgCl2 are both good conductors and are ionic in nature whereas the rest in period 3 are covalent in nature and don't conduct. True or false?

Select one of the following:

True
False

Explanation

Question 26 of 31

1

Which definition of 1st Ionisation Energy and Electronegativity is correct?

Select one of the following:

1st Ionisation Energy = minimum energy required to remove 1 mole of gaseous electrons from 1 mole of gaseous atoms
Electronegativity = ability of an atom to attract electrons in a ionic bond
1st Ionisation Energy = minimum energy required to remove 1 mole of gaseous electrons from 1 mole of gaseous atoms
Electronegativity = ability of an atom to attract electrons in a covalent bond

Explanation

Question 27 of 31

1

An transition element is:
an element that possesses an incomplete or sub-level in one or more of its oxidation states

Select one of the following:

True
False

Explanation

Question 28 of 31

4

Tick the correct properties of transition elements

Select one or more of the following:

Variable oxidation number
complex ion formation
Catalyst properties
Coloured complexes

Explanation

Question 29 of 31

2

Why are Sc and Zn not considered as transitional metals?

Select one or more of the following:

Sc not transition metal as its common ion Sc³⁺ has no d electrons
Zinc not transition metal as contains full d sub level in all oxidation states
Zinc not transition metal as contains has no full d sub level in all oxidation states

Explanation

Question 30 of 31

1

What is a ligand?

Select one of the following:

Species that uses a lone pair of electrons to form dative covalent bonds with a non-metal ion.
Species that possesses an incomplete or sub-level in one or more of its oxidation states
Species that uses a lone pair of electrons to form dative covalent bonds with a metal ion.
Species which is the arrangement showing the properties of elements repeat periodically

	Created by hanalou about 10 years ago

Questions orientated around periodicity in IB Chemistry (SL = questions 1 - 26; HL= all questions)

Periodicity

Periodicity

Question 1 of 31

Describe the electronegativity and atomic radius trend across a period

Select one of the following:

Explanation

Question 2 of 31

Melting point increases across a period

Select one of the following:

Explanation

Question 3 of 31

non-metals have a giant molecular structure meaning a lot of energy is required to break the bonds

Select one of the following:

Explanation

Question 4 of 31

Which two answers correctly describe electrical conductivity

Select one or more of the following:

Explanation

Question 5 of 31

Ionic radius decreases across the period until formation of the negative ions. Afterwards there is a sudden increase followed by a steady decrease to the end. Is this true or false?

Select one of the following:

Explanation

Question 6 of 31

Why does sulphur have a higher melting point than phosphorous?

Select one or more of the following:

Explanation

Question 7 of 31

Which physical property increases down a group but decreases across a period

Select one of the following:

Explanation

Question 8 of 31

Why are there no values for atomic radius for noble gases? (two answers)

Select one or more of the following:

Explanation

Question 9 of 31

Which is the correct order of decreasing radii for Cl, Cl+, Cl- ?

Select one of the following:

Explanation

Question 10 of 31

What are the chemical properties of Group 0 (Noble gases)?

Select one of the following:

Explanation

Question 11 of 31

What are the chemical properties of Group 1 (alkali metals)?

Select one of the following:

Explanation

Question 12 of 31

Halogens reactivity increases down a group, they form ionic compounds with metals or covalently with non-metals, have 6 in the outer shell, diotomic

Select one of the following:

Explanation

Question 13 of 31

There is no displacement reaction in this equation because Iodine is weaker than Bromine 2KBr + I2 ----->

Select one of the following:

Explanation

Question 14 of 31

What are the characteristics of chlorides? (tick three)

Select one or more of the following:

Explanation

Question 15 of 31

'Increasing charge density of the positive ion polarises the chloride ion as we move to the right hand side'. Is this true?

Select one of the following:

Explanation

Question 16 of 31

Here is a list describing and explaining the melting point trend across period 3. Which one is INCORRECT

Select one or more of the following:

Explanation

Question 17 of 31

Which oxides are insoluble in water?

Select one or more of the following:

Explanation

Question 18 of 31

Which oxides DO NOT react with HCl?

Select one or more of the following:

Explanation

Question 19 of 31

Which ones react when NaOH is added?

Select one or more of the following:

Explanation

Question 20 of 31

Ionic radius decreases across the period until formation of the negative ions. Afterwards there is a sudden increase followed by a steady decrease to the end.

Is this true or false?

There is no displacement reaction in this equation because Iodine is weaker than Bromine

2KBr + I2 ----->

An transition element is:
an element that possesses an incomplete or sub-level in one or more of its oxidation states