Metallic bonding is the electrostatic attraction between:
Cations and delocalised electrons
Two shared electron pairs
Oppositely charged ions
Neutral atoms
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WhyMetallic bonding is the attraction between a lattice of positive metal ions (cations) and a sea of delocalised valence electrons.
2Multiple choice · Easy
Why do metals conduct electricity?
They contain mobile delocalised electrons
They contain mobile ions
They have shared electron pairs
They are very dense
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WhyMetals contain delocalised (mobile) electrons that are free to move through the lattice and carry charge.
3Multiple choice · Medium
Which factor strengthens metallic bonding?
A higher cation charge and smaller radius
A lower charge and larger radius
Fewer delocalised electrons
Neutral atoms in the lattice
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WhyMetallic bond strength increases with greater ionic charge (more delocalised electrons) and a smaller cation radius.
4Multiple choice · Medium
Why are metals malleable?
Layers of cations can slide over one another
They contain weak covalent bonds
The ions are held rigidly
They have no bonding
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WhyThe layers of cations can slide over one another while the delocalised electrons continue to hold the structure together, so the metal can be hammered into shape without shattering.
5Multiple choice · Medium
Which of these period 3 metals has the strongest metallic bonding?
Sodium
Magnesium
Aluminium
They are all equal
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Why$\text{Al}^{3+}$ has the highest charge and contributes 3 delocalised electrons per atom, giving the strongest metallic bonding of Na, Mg and Al.
6Multiple choice · Hard
What is the trend in melting point across the period 3 metals Na, Mg and Al?
Increases from Na to Al
Decreases from Na to Al
Stays the same
Increases then decreases
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WhyMelting point increases Na $<$ Mg $<$ Al because the charge on the cation and the number of delocalised electrons both increase, strengthening the metallic bonding.
7Fill in the blank · Easy
In metallic bonding the valence electrons are described as because they are free to move throughout the lattice.
Answer:
delocalised / delocalized / mobile
WhyThe electrons are delocalised (not associated with any one atom), forming a sea of electrons.
8Fill in the blank · Medium
In metallic sodium each atom contributes one electron to the electron sea and becomes a cation with charge (give sign and number).
Answer:
1+ / +1
WhySodium is in group 1, so it loses its single valence electron to become $\text{Na}^{+}$.
9Multiple choice · Medium
Why are alloys generally harder than the pure metal?
Different-sized atoms distort the layers, making them harder to slide
Alloys contain covalent bonds
Alloys have no delocalised electrons
Alloys are ionic compounds
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WhyAtoms of different sizes disrupt the regular lattice, making it harder for layers to slide over one another.
10Multiple choice · Easy
Metallic bonding is best described as
positive ions attracted to a sea of delocalised electrons
shared pairs of electrons between atoms
oppositely charged ions in a lattice
molecules held by hydrogen bonds
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WhyMetallic bonding is electrostatic attraction between positive metal ions and a sea of delocalised electrons.
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