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Gases

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Questions orientated around periodicity in IB Chemistry (SL = questions 1 - 26; HL= all questions)
Kylie Ariana
Quiz by Kylie Ariana, updated more than 1 year ago More Less
hanalou
Created by hanalou almost 11 years ago
Saeed Al hefaity
Copied by Saeed Al hefaity almost 8 years ago
Kylie Ariana
Copied by Kylie Ariana over 7 years ago
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Resource summary

Question 1

Question
Describe the electronegativity and atomic radius trend across a period
Answer
  • 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

Question 2

Question
Melting point increases across a period
Answer
  • True
  • False

Question 3

Question
non-metals have a giant molecular structure meaning a lot of energy is required to break the bonds
Answer
  • True
  • False

Question 4

Question
Which two answers correctly describe electrical conductivity
Answer
  • 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

Question 5

Question
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?
Image:
WP_000803 (image/jpg)
Answer
  • True
  • False

Question 6

Question
Why does sulphur have a higher melting point than phosphorous?
Answer
  • there are higher intermolecular forces between sulphur than phosphorous
  • there are lower intermolecular forces between sulphur than phosphorous

Question 7

Question
Which physical property increases down a group but decreases across a period
Answer
  • Ionic radius
  • Atomic radius
  • Electronegativity

Question 8

Question
Why are there no values for atomic radius for noble gases? (two answers)
Answer
  • The atomic radius doesn't affect their nuclear charge
  • Nuclei distance is difficult to measure
  • They do not generally bond to other atoms

Question 9

Question
Which is the correct order of decreasing radii for Cl, Cl+, Cl- ?
Answer
  • Cl, Cl-, Cl+
  • Cl+, Cl, Cl-
  • Cl-, Cl+, Cl
  • Cl-. Cl, Cl+

Question 10

Question
What are the chemical properties of Group 0 (Noble gases)?
Answer
  • odour, colourless, mono atomic, reactive
  • odourless, colourless, mono atomic, unreactive
  • odourless, colour, not mono atomic, unreactive
  • odour, colour, not mono atomic, reactive

Question 11

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

Question 12

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

Question 13

Question
There is no displacement reaction in this equation because Iodine is weaker than Bromine 2KBr + I2 ----->
Answer
  • True
  • False

Question 14

Question
What are the characteristics of chlorides? (tick three)
Answer
  • Na, Mg - alkaline
  • Al - amphoteric
  • Si, P, S, Cl - alkaline
  • Si, P, S, Cl - acidic
  • Na, Mg - acidic

Question 15

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

Question 16

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

Question 17

Question
Which oxides are insoluble in water?
Answer
  • Na2O
  • MgO
  • Al2O3
  • SiO2
  • P4O10 (or P4O6)
  • SO3 (or SO2)
  • Cl2O7 Cl2O

Question 18

Question
Which oxides DO NOT react with HCl?
Answer
  • Na2O
  • SO3 (OR SO2)
  • Al2O3
  • P4O10 (OR P4O6)
  • SiO2
  • MgO
  • Cl2O7 Cl2O

Question 19

Question
Which ones react when NaOH is added?
Answer
  • Na2O
  • MgO
  • SiO2
  • H3PO4
  • SO2
  • HCl2O7
  • Al2O3

Question 20

Question
Oxides in period 3 are either Basic Oxide, Amphoteric Oxide or Acidic Oxide
Answer
  • True
  • False

Question 21

Question
Which ones have a good conductivity? (3 answers)
Answer
  • Na2O
  • Al2O7
  • SiO2
  • P4O10
  • MgO
  • Cl2O7

Question 22

Question
Melting point in period 3 oxides increases Na2O --> MgO and then decreases from MgO ---> Cl2O7
Answer
  • True
  • False

Question 23

Question
Which chlorides across period 3 dissolves in water?
Answer
  • NaCl
  • Al2Cl6
  • SiCl4
  • MgCl2
  • PCl3
  • PCl5
  • Cl2

Question 24

Question
Melting point increases across period 3 chlorides
Answer
  • True
  • False

Question 25

Question
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?
Answer
  • True
  • False

Question 26

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

Question 27

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

Question 28

Question
Tick the correct properties of transition elements
Answer
  • Variable oxidation number
  • complex ion formation
  • Catalyst properties
  • Coloured complexes

Question 29

Question
Why are Sc and Zn not considered as transitional metals?
Answer
  • 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

Question 30

Question
What is a ligand?
Answer
  • 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

Question 31

Question
Why are some of the complexes of the d-block elements coloured?
Answer
  • energy difference between levels corresponds to particular wavelength of light
  • because they are
  • colour produced complement to wavelength absorbed when electrons excited.
  • electron transitions (electron jumps) from one orbital to another
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