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Questions and Answers
What is the primary characteristic of lattice enthalpy?
What is the primary characteristic of lattice enthalpy?
The activation energy is the maximum energy required for a reaction to occur.
The activation energy is the maximum energy required for a reaction to occur.
False
What effect does an increase in temperature have on the rate of reaction?
What effect does an increase in temperature have on the rate of reaction?
It increases the rate of reaction.
A ___________ catalyst is in the same phase as the reactants.
A ___________ catalyst is in the same phase as the reactants.
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Match the terms related to reaction rates with their definitions:
Match the terms related to reaction rates with their definitions:
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Which statement is true regarding enzymes?
Which statement is true regarding enzymes?
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Increasing the concentration of reactants decreases the rate of reaction.
Increasing the concentration of reactants decreases the rate of reaction.
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What is the effect of a catalyst on activation energy?
What is the effect of a catalyst on activation energy?
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What is the first ionization energy?
What is the first ionization energy?
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Electronegativity increases as atomic size decreases.
Electronegativity increases as atomic size decreases.
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Define hybridization in chemistry.
Define hybridization in chemistry.
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The ______ reaction releases heat to its surroundings.
The ______ reaction releases heat to its surroundings.
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Match the following types of bonds with their characteristics:
Match the following types of bonds with their characteristics:
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What factor increases the strength of metallic bonding?
What factor increases the strength of metallic bonding?
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The bond energy is the energy required to break one mole of covalent bonds in the gaseous state.
The bond energy is the energy required to break one mole of covalent bonds in the gaseous state.
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What is the trend of ionization energy across a period?
What is the trend of ionization energy across a period?
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The standard enthalpy change of combustion (ΔHc^⦵^) is when one mole of a substance is burnt in excess ______.
The standard enthalpy change of combustion (ΔHc^⦵^) is when one mole of a substance is burnt in excess ______.
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Match the following types of enthalpy changes with their definitions:
Match the following types of enthalpy changes with their definitions:
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Which of the following is not a factor affecting ionization energy?
Which of the following is not a factor affecting ionization energy?
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Hydrogen bonding is a type of dipole-dipole interaction.
Hydrogen bonding is a type of dipole-dipole interaction.
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What is Hess's Law?
What is Hess's Law?
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In a molecule with two bond pairs and two lone pairs, the shape is ______.
In a molecule with two bond pairs and two lone pairs, the shape is ______.
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What happens to the atomic radius as nuclear charge increases?
What happens to the atomic radius as nuclear charge increases?
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Study Notes
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.
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Description
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!
