Chemistry Revision Flashcards

A collection of flashcards based on multiple choice questions and concepts related to chemistry for effective revision and exam preparation.

What best describes the structure of a solid ionic compound?

Positive and negative ions arranged in a regular crystal lattice.

What ion is formed by potassium when it reacts with bromine?

K⁺.

Which property is NOT typical of ionic compounds?

They have low melting points.

Why are ionic compounds brittle?

Layers shift so like charges align, causing repulsion and shattering.

Why do ionic compounds dissolve in water?

Water molecules surround and stabilize the separate ions (hydration).

What is the charge of the oxide ion formed when oxygen gains electrons?

2−.

Which molecule contains a double covalent bond?

O₂.

Why is the molecule F₂ non-polar?

Its two identical atoms share electrons equally.

How many bonding pairs and lone pairs does Cl₂ have in total?

1 bonding pair, 3 lone pairs.

What is a typical property of small, non-polar covalent molecules?

Low boiling point and poor electrical conductivity.

In which molecule does the central atom carry a partial positive charge (δ+)?

HF.

Which of the following is a polar molecule despite having polar bonds?

NH₃.

What does an electronegativity difference of 1.2 between two bonded atoms indicate?

Polar covalent bond.

What is correct about a polar bond?

One atom has a partial positive charge and the other a partial negative charge.

Why do metals have high thermal conductivity?

Ions vibrate and pass kinetic energy through delocalized electrons.

What factor causes metals to have a lustrous appearance?

Delocalized electrons reflecting light.

Which metal would you expect to have the highest melting point?

Aluminium (3 delocalized e⁻ per atom).

Why can metals be drawn into wires?

Metal ions can slide past each other while the electron sea maintains cohesion.

Which molecule exhibits hydrogen bonding with itself?

HF.

Why does boiling point increase with chain length in non-polar hydrocarbons?

London dispersion forces increase with more electrons and greater surface area.

Which pair of molecules exhibit dipole-dipole interactions but not hydrogen bonding?

HCl and HCl.

Why is ice less dense than liquid water?

Hydrogen bonds hold molecules in a more open, hexagonal lattice structure.

What type of intermolecular force exists between all molecules?

London dispersion forces.

What is the correct formula for iron(II) sulfate?

FeSO₄.

Which formula correctly represents tin(IV) oxide?

SnO₂.

What is the formula of ammonium phosphate?

(NH₄)₃PO₄.

What is the name of the compound with the formula Pb(NO₃)₂?

Lead(II) nitrate.

How do gas particles move?

Particles move rapidly and randomly, filling the container.

What is the temperature at which a substance changes from liquid to gas called?

Boiling point.

Which change of state requires energy to be released from the substance?

Condensation.

Ionic compounds in the __________ state conduct electricity because their ions are free to move. (Fill in the blank)

molten.

The bond in H₂ is described as __________ covalent. (Fill in the blank)

non-polar.

The VSEPR theory predicts that the shape of BF₃ is __________ planar. (Fill in the blank)

trigonal.

In metallic bonding, the force of attraction is between positive __________ and delocalized electrons. (Fill in the blank)

cations.

The unusually high boiling point of water compared to H₂S is due to __________ bonding. (Fill in the blank)

hydrogen.

The formula for cobalt(III) nitrate is __________. (Fill in the blank)

Co(NO₃)₂.

The process of a liquid turning into a gas below its boiling point is called __________. (Fill in the blank)

evaporation.

A molecule is non-polar overall when its polar bonds are arranged __________. (Fill in the blank)

symmetrically.

The strength of London dispersion forces depends on the number of __________. (Fill in the blank)

electrons.

The name of the compound Cr₂O₃ is chromium(III) __________. (Fill in the blank)

oxide.

When an ionic compound dissolves in water, the resulting solution conducts electricity. (True/False) Correct if False.

True.

A molecule of CO₂ has polar bonds but is a non-polar molecule overall. (True/False) Correct if False.

True.

Metallic bonds are directional, which is why metals are brittle. (True/False) Correct if False.

False; Metallic bonds are non-directional, allowing metals to be malleable.

The boiling point of noble gases increases as you go down Group 18. (True/False) Correct if False.

True.

Dipole-dipole forces are stronger than hydrogen bonds. (True/False) Correct if False.

False; Hydrogen bonds are stronger than dipole-dipole forces.

In the solid state, the particles of a substance have zero kinetic energy. (True/False) Correct if False.

False; Particles have low kinetic energy, but not zero.

The formula for lead(IV) oxide is PbO₂. (True/False) Correct if False.

True.

Network covalent solids (e.g. diamond) have low melting points. (True/False) Correct if False.

False; They have high melting points.

London dispersion forces are present in polar molecules as well as non-polar ones. (True/False) Correct if False.

True.

An ammonium ion (NH₄⁺) acts as a cation in ionic compounds. (True/False) Correct if False.

True.

What is the ionic formula for Lithium (Li⁺) and Nitrogen (N³⁻)?

Li₃N.

What is the ionic formula for Strontium (Sr²⁺) and Bromide (Br⁻)?

SrBr₂.

What is the ionic formula for Aluminum (Al³⁺) and Oxide (O²⁻)?

Al₂O₃.

What is the ionic formula for Silver (Ag⁺) and Iodide (I⁻)?

AgI.

What is the ionic formula for Cobalt(II) (Co²⁺) and Sulfide (S²⁻)?

CoS.

What is the ionic formula for Tin(IV) (Sn⁴⁺) and Chloride (Cl⁻)?

SnCl₄.

What is the ionic formula for Mercury(II) (Hg²⁺) and Oxide (O²⁻)?

HgO.

What is the ionic formula for Vanadium(III) (V³⁺) and Fluoride (F⁻)?

VF₃.

What is the ionic formula for Barium (Ba²⁺) and Nitrate (NO₃⁻)?

Ba(NO₃)₂.

What is the ionic formula for Potassium (K⁺) and Carbonate (CO₃²⁻)?

K₂CO₃.

What is the ionic formula for Aluminum (Al³⁺) and Sulfate (SO₄²⁻)?

Al₂(SO₄)₃.

What is the ionic formula for Ammonium (NH₄⁺) and Phosphate (PO₄³⁻)?

(NH₄)₃PO₄.

What is the ionic formula for Sodium (Na⁺) and Hydroxide (OH⁻)?

NaOH.

What is the ionic formula for Calcium (Ca²⁺) and Nitrate (NO₃⁻)?

Ca(NO₃)₂.

What is the ionic formula for Iron(III) (Fe³⁺) and Nitrate (NO₃⁻)?

Fe(NO₃)₃.

What is the ionic formula for Copper(II) (Cu²⁺) and Carbonate (CO₃²⁻)?

CuCO₃.

What is the ionic formula for Manganese(II) (Mn²⁺) and Phosphate (PO₄³⁻)?

Mn3(PO₄)₂.

What is the ionic formula for Chromium(III) (Cr³⁺) and Sulfate (SO₄²⁻)?

Cr₂(SO₄)₃.

What is the ionic formula for Lead(II) (Pb²⁺) and Hydroxide (OH⁻)?

Pb(OH)₂.

What is the ionic formula for Cobalt(III) (Co³⁺) and Carbonate (CO₃²⁻)?

Co₂(CO₃)₃.