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Periodicity Flashcards | StudBud
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Periodicity
Periodicity
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Flashcards
15 cards
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Practice quiz
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Questions
15
Answers
1
Nitrogen has a lower ionisation energy than Oxygen.
False
True
2
silicon, graphite and diamond are all made up of carbon atoms in a tetrahedral shape.
True
False
3
silicon, graphite and diamond are examples of a...?
flavour of icecream
giant covalent lattice
giant ionic lattice
giant metallic lattice
4
what makes metallic bonding strong?
permanent dipoles between cations and anions
intra molecular forces
electrostatic attraction
inter molecular forces
5
What's Ruby's favorite thing to do?
Sleep
Eat
All of the above
Read
6
which metal is a liquid at room temperature
Mecury
None they're metals and have strong bonds
Boron
If you're in the desert it's hot enough so they all melt
7
across periods 2 and 3 the sharp decrease in melting points is because...?
change from simple to giant molecular structures
change from giant to simple molecular structures
8
How does Ruby feel about chemistry?
'glass half full'
'we're all going to fail'
Loves it
It's better than Biology
9
How are the elements arranged in the periodic table?
By increasing atomic number
By alphabetical order
By colour co-ordination
increases the atomic radius
10
what's the name of the elements in group 2?
alkali metals
alkaline earth metals
alkali earth metals
alkaline metals
11
The fall in ionisation energy from beryllium to boron is because of what?
the start of filling the 2p sub-shell
increased electron shielding
an accident
It's not a fall there's a rise
12
Diatomic gases have weak forces between molecules, the bonds in the molecules are strong and..?
Purely Covalent
Purely Ionic
13
An element has as many ionisation energies as electrons.
False
True
14
Carbon is a good electrical conductor when in planar hexagonal layers because...?
There's a sea of delocalised electrons
It's a metal
Who cares I've finally finished the quiz
only three of the outer electrons are covalently bonded
15
What measures how easily an atom loses an electron to form a positive ion?
First ionisation energy
second ionisation energy
enthalpy change of formation
enthalpy change of reaction
