SQA Higher Chemistry Area 1 Chemical Changes and Structure overview quiz quiz

In order of increasing atomic number

In order of increasing relative atomic mass

In order of decreasing reactivity

Alphabetically by name

It increases because extra electron shells are added one after another as you move across the period

It decreases because the increasing nuclear charge pulls the same shell of electrons closer

It stays exactly the same right across the period

It first increases steadily and then decreases towards the end

Relative atomic mass, the density of the solid and the colour of the element

The temperature, the pressure and the concentration of the surrounding solution

Nuclear charge, number of occupied shells and screening by inner electrons

The bond length, the bond angle and the bond enthalpy of the molecule

It increases steadily as you move further down the group towards the heavier elements

It stays constant all the way down the group

It depends only on the relative atomic mass of the element

It decreases because the outer electron is further out and more screened

Hydrogen bonding

London dispersion forces

Permanent dipole-permanent dipole interactions

Metallic bonding

The strong covalent bonds holding the atoms together inside each molecule

The intermolecular forces between the molecules

The nuclear attraction between protons and electrons

The giant ionic lattice of the solid

The gain of electrons

The gain of protons

The loss of electrons

The loss of neutrons

The total masses of the reactants in each half-equation must be exactly equal

Both of the half-equations being combined must be reduction reactions

The reaction temperatures of the two half-equations must match

The number of electrons lost must equal the number of electrons gained

An unstable, high-energy arrangement of atoms at the top of the energy barrier

A stable final product of the reaction that forms once the barrier has been crossed completely

A catalyst that lowers the activation energy of the reaction

The reactant molecule that happens to have the lowest energy

By raising the temperature of the reactant mixture so the particles move faster

By providing an alternative pathway with a lower activation energy

By increasing the activation energy of the reaction

By being used up as one of the reactants is consumed

It lowers the activation energy that is needed for each collision to be successful

It changes the overall enthalpy change of the reaction itself

There are more particles per unit volume, so collisions are more frequent

It denatures the reactant particles in the mixture

Oxygen

Chlorine

Caesium

Fluorine