Describe the electronegativity and atomic radius trend across a period
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
Melting point increases across a period
non-metals have a giant molecular structure meaning a lot of energy is required to break the bonds
Which two answers correctly describe electrical conductivity
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
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?
Why does sulphur have a higher melting point than phosphorous?
there are higher intermolecular forces between sulphur than phosphorous
there are lower intermolecular forces between sulphur than phosphorous
Which physical property increases down a group but decreases across a period
Ionic radius
Atomic radius
Electronegativity
Why are there no values for atomic radius for noble gases? (two answers)
The atomic radius doesn't affect their nuclear charge
Nuclei distance is difficult to measure
They do not generally bond to other atoms
Which is the correct order of decreasing radii for Cl, Cl+, Cl- ?
Cl, Cl-, Cl+
Cl+, Cl, Cl-
Cl-, Cl+, Cl
Cl-. Cl, Cl+
What are the chemical properties of Group 0 (Noble gases)?
odour, colourless, mono atomic, reactive
odourless, colourless, mono atomic, unreactive
odourless, colour, not mono atomic, unreactive
odour, colour, not mono atomic, reactive
What are the chemical properties of Group 1 (alkali metals)?
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
Halogens reactivity increases down a group, they form ionic compounds with metals or covalently with non-metals, have 6 in the outer shell, diotomic
There is no displacement reaction in this equation because Iodine is weaker than Bromine
2KBr + I2 ----->
What are the characteristics of chlorides? (tick three)
Na, Mg - alkaline
Al - amphoteric
Si, P, S, Cl - alkaline
Si, P, S, Cl - acidic
Na, Mg - acidic
'Increasing charge density of the positive ion polarises the chloride ion as we move to the right hand side'. Is this true?
Here is a list describing and explaining the melting point trend across period 3. Which one is INCORRECT
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
Which oxides are insoluble in water?
Na2O
MgO
Al2O3
SiO2
P4O10 (or P4O6)
SO3 (or SO2)
Cl2O7 Cl2O
Which oxides DO NOT react with HCl?
SO3 (OR SO2)
P4O10 (OR P4O6)
Which ones react when NaOH is added?
H3PO4
SO2
HCl2O7
Oxides in period 3 are either Basic Oxide, Amphoteric Oxide or Acidic Oxide
Which ones have a good conductivity? (3 answers)
Al2O7
P4O10
Cl2O7
Melting point in period 3 oxides increases Na2O --> MgO and then decreases from MgO ---> Cl2O7
Which chlorides across period 3 dissolves in water?
NaCl
Al2Cl6
SiCl4
MgCl2
PCl3
PCl5
Cl2
Melting point increases across period 3 chlorides
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?
Which definition of 1st Ionisation Energy and Electronegativity is correct?
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
An transition element is: an element that possesses an incomplete or sub-level in one or more of its oxidation states
Tick the correct properties of transition elements
Variable oxidation number
complex ion formation
Catalyst properties
Coloured complexes
Why are Sc and Zn not considered as transitional metals?
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
What is a ligand?
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
Why are some of the complexes of the d-block elements coloured?
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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