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CfE Higher Chemistry - Periodicity Flashcards | StudBud
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CfE Higher Chemistry - Periodicity
CfE Higher Chemistry - Periodicity
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Trends of the periodic table - ionisation energy, electronegativity and covalent radius.
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Questions
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Answers
1
What happens to electronegativity going
ACROSS
the Periodic Table?
Increases
Stays the same.
Decreases
2
What happens to ionisation energy going
ACROSS
the Periodic Table?
Increases
Decreases
Stays the same
3
What happens to covalent radius going
DOWN
a group of the Periodic Table?
Stays the same
Decreases
Increases
4
Why are fluorine atoms smaller than lithium atoms?
Fluorine has a greater electronegativity.
Fluorine has more protons in its nucleus.
Lithium has a greater number of energy levels.
5
Which of the following has a monatomic structure?
Carbon
Neon
Silicon
Nitrogen
6
Which is the equation for the second ionisation energy of calcium?
Ca (s) -> Ca+ (g) + e-
Ca+(g) -> Ca2+ (g) + e-
Ca+ (g) + e- -> Ca (g)
Ca (g) -> Ca+ (g) + e-
7
Which is the equation for the first ionisation energy of aluminium?
Al+ (g) + e- -> Al (g)
Al (g) -> Al+ (g) + e-
Al (s) -> Al+ (g) + e-
Al+(g) -> Al2+ (g) e-
8
High electronegativity means...
Weak attraction for bonding electrons.
Strong attraction for the nucleus.
Strong attraction for bonding electrons.
Weak attraction for the nucleus.
9
What kind of bonding holds a atoms in a sample of aluminium together?
Ionic
Metallic
Covalent molecular
Covalent network
10
Why is there such an increase between the second and third ionisation energies of calcium?
Calcium atoms have a larger nuclear charge.
There is a shielding effect.
The third electron must be removed from a full shell.
