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Questions and Answers
What is the energy required to remove the first electron from a neutral atom?
What is the energy required to remove the first electron from a neutral atom?
What happens to ionization energy as you move down a group in the periodic table?
What happens to ionization energy as you move down a group in the periodic table?
What is the main factor that influences the formation of ionic bonds between atoms?
What is the main factor that influences the formation of ionic bonds between atoms?
What is the result of increased nuclear charge on ionization energy?
What is the result of increased nuclear charge on ionization energy?
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What is the effect of increased shielding by inner electrons on ionization energy?
What is the effect of increased shielding by inner electrons on ionization energy?
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What is a key factor that determines an atom's chemical reactivity?
What is a key factor that determines an atom's chemical reactivity?
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What is formed by combining atomic orbitals?
What is formed by combining atomic orbitals?
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What determines the molecular shape of a molecule?
What determines the molecular shape of a molecule?
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What is the purpose of VSEPR theory?
What is the purpose of VSEPR theory?
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What is the unit of amount of substance?
What is the unit of amount of substance?
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What is the molar mass of a substance?
What is the molar mass of a substance?
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What is percent composition?
What is percent composition?
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What is the purpose of stoichiometric calculations?
What is the purpose of stoichiometric calculations?
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What is the limiting reagent?
What is the limiting reagent?
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Study Notes
Ionization Energy
Definition
Ionization energy is the energy required to remove an electron from a neutral atom or molecule in its ground state.
Key Concepts
- First Ionization Energy (IE1): energy required to remove the first electron from a neutral atom
- Successive Ionization Energies (IE2, IE3, ...): energies required to remove subsequent electrons from the resulting ion
Trends
- Increase across a period: ionization energy increases as you move from left to right across a period due to increased nuclear attraction and decreased atomic size
- Decrease down a group: ionization energy decreases as you move down a group due to increased atomic size and shielding of the nucleus by inner electrons
Factors Affecting Ionization Energy
- Nuclear Charge: increased nuclear charge increases ionization energy
- Atomic Size: smaller atomic size increases ionization energy
- Shielding: increased shielding by inner electrons decreases ionization energy
Importance of Ionization Energy
- Determines chemical reactivity: ionization energy influences an atom's ability to gain or lose electrons, affecting its reactivity
- Affects ionic bond formation: ionization energy influences the formation of ionic bonds between atoms with different ionization energies
Ionization Energy
Definition
- Energy required to remove an electron from a neutral atom or molecule in its ground state.
Key Concepts
- First Ionization Energy (IE1): energy required to remove the first electron from a neutral atom.
- Successive Ionization Energies (IE2, IE3,...): energies required to remove subsequent electrons from the resulting ion.
Trends
- Ionization energy increases as you move from left to right across a period due to increased nuclear attraction and decreased atomic size.
- Ionization energy decreases as you move down a group due to increased atomic size and shielding of the nucleus by inner electrons.
Factors Affecting Ionization Energy
- Increased nuclear charge increases ionization energy.
- Smaller atomic size increases ionization energy.
- Increased shielding by inner electrons decreases ionization energy.
Importance of Ionization Energy
- Ionization energy influences an atom's ability to gain or lose electrons, affecting its reactivity.
- Ionization energy influences the formation of ionic bonds between atoms with different ionization energies.
Molecular Structure
- Atomic orbitals are regions around an atom where an electron is likely to be found, which influence molecular shape.
- Molecular orbitals are formed by combining atomic orbitals, describing the distribution of electrons within a molecule.
Bonding Theories
- VSEPR Theory predicts molecular shape based on electron pair repulsion, considering both bonding and non-bonding pairs.
- MO Theory describes molecular structure and bonding in terms of molecular orbitals, providing a more detailed understanding of molecular interactions.
Molecular Shape
- Linear shape occurs when a central atom has two bonding pairs and no non-bonding pairs.
- Trigonal planar shape occurs when a central atom has three bonding pairs and no non-bonding pairs.
- Tetrahedral shape occurs when a central atom has four bonding pairs and no non-bonding pairs.
- Bent shape occurs when a central atom has two bonding pairs and one non-bonding pair.
Stoichiometry
- Stoichiometry studies the quantitative relationships between reactants and products in chemical reactions.
- A mole is a unit of amount of substance, defined as 6.022 x 10^23 particles (atoms or molecules).
- Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol).
Composition of Compounds
- Empirical formula represents the simplest whole-number ratio of atoms in a compound.
- Molecular formula represents the actual number of atoms in a molecule.
- Percent composition is the percentage of each element in a compound by mass.
Stoichiometric Calculations
- Mole ratios are used to calculate the amount of reactants required or products formed.
- The limiting reagent is the reactant that determines the amount of product formed.
- Percent yield is the actual yield of a reaction compared to the theoretical yield, expressed as a percentage.
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Description
Ionization energy quiz covering key concepts such as first ionization energy, successive ionization energies, and trends across periods.
