Atomic Structure and Periodic Trends Quiz

Atomic Structure

• Electrons have a charge of -1 and are very small.
• Nuclei are positively charged.
• 1 picometer = 1 x 10^-12 meter.

Factors Affecting Atomic Radius

• Increasing nuclear charge decreases atomic radius.
• Increased shielding effect increases atomic radius.

Periodic Trends

• Atomic size increases down a group (more shielding effect).
• Atomic size decreases across a period (more effective nuclear charge).

Ionic Charge

• Ions in the same group have the same charge.

Ionic Size

• Ionic radius increases to the left and down within cations and anions.
• Cations are smaller than their neutral atom.
• Anions are larger than their neutral atom.

Ionisation Energy

• First ionization energy is the energy needed to remove one electron from a gas atom.
• Second ionization energy is the energy needed to remove an electron from a unipositive ion.
• Ionization energy increases across a period and decreases down a group.

Electronegativity

• Electronegativity is the ability of an atom to attract a pair of electrons in a covalent bond.
• Electronegativity increases across a period and decreases down a group.

Bonding

• Ionic Bonding: Occurs between metals and non-metals.
• Covalent Bonding: Occurs between non-metals.
• Dative/Co-ordinate Bonding: A covalent bond where both electrons in the shared pair come from the same atom.
• Metallic Bonding: Occurs between metals.

Factors Affecting Metallic Bonds

• Increasing number of delocalized electrons increases metallic bonding.
• Increasing charge of an ion increases metallic bonding.
• Increasing ionic size decreases metallic bonding.

Types of Hybridisation

• Sigma Bonds: Formed by end-on overlap of orbitals; strong bond.
• Pi Bonds: Formed by lateral overlap of orbitals; weaker than sigma bonds.

Factors Affecting Reactivity of Molecules

• Bond strength: Stronger bonds increase reactivity.
• Polarity: Influence reactivity.

Shapes of Molecules

• Molecule shapes are determined by the repulsion between electron pairs.

Factors Affecting Rate of Reaction

• Concentration: Higher concentration leads to more collisions and faster reaction rates.
• Pressure: Higher pressure leads to more collisions and faster reaction rates.
• Surface area: Larger surface area leads to more collisions and faster reaction rates.
• Temperature: Higher temperature leads to more collisions and faster reaction rates.
• Catalysts: Catalysts speed up reactions by providing an alternative pathway with a lower activation energy.

Maxwell-Boltzmann Distribution

• Depicts the distribution of particle energies in a sample of matter.
• Activation energy is the minimum energy particles need for reaction.

Types of Catalysts

• Homogeneous Catalysts: The Catalyst is in the same phase as the reactants.
• Heterogeneous Catalysts: The Catalyst is in a different phase from the reactants.

Measuring Rate of Reaction

• Rate equation linking rate and reactant concentration.
• Order reaction: Indicates how reaction rate is affected by concentration.

First, Second, and Zero Order Reactions

• First order: Doubling reactant concentration doubles reaction rate.
• Second order: Doubling reactant concentration quadruples reaction rate.
• Zero order: Changing reactant concentration doesn't affect reaction rate.

Born-Haber Cycle

• Used to calculate the enthalpy change of formation of ionic compounds.
• A series of steps, with different enthalpy changes, which can be calculated to find enthalpy change of formation.

Enthalpy Changes

• Enthalpy change of a reaction is the energy absorbed or released.
• Standard conditions define conditions under which enthalpy change is measured.

Enthalpy of Formation

• Measuring the enthalpy needed to form one mole of a compound from its elements.

Electron Affinity

• Electron affinity is the energy change when an electron is added to a neutral gaseous atom.

Enthalpy of Atomisation

• Standard enthalpy change for breaking one mole of bonds.

Test your knowledge on atomic structure, factors affecting atomic radius, and periodic trends. This quiz covers key concepts such as electronegativity, ionic charge, and ionization energy. Challenge yourself and see how well you understand the fundamentals of atomic theory!