Chemistry Atomic Structure Trends
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Questions and Answers

What happens to the atomic radius as you move across a period?

  • Atomic radius fluctuates unpredictably
  • Atomic radius decreases (correct)
  • Atomic radius increases
  • Atomic radius remains constant

    • All nitrates are insoluble.

    False

    What is the significance of the M+1 peak in mass spectrometry?

    It indicates the presence of carbon-13 isotopes in the organic compound.

    In the molecular formula calculation, the molecular formula = empirical formula x Mr of __________ / Mr of the empirical formula.

    <p>the compound</p> Signup and view all the answers

    Match the following ions with their properties:

    <p>Cl = Has two isotopes, 35Cl and 37Cl Ag = Forms insoluble compounds with halides K = Forms soluble salts with nitrates Ba = Has limited solubility in sulfates</p> Signup and view all the answers

    Which of the following represents the correct outcome of the precipitation reaction between silver nitrate and sodium chloride?

    <p>AgCl forms as a solid</p> Signup and view all the answers

    The height of the M+1 peak decreases with an increase in the number of carbon atoms in a molecule.

    <p>False</p> Signup and view all the answers

    What does the term 'ionic bond' refer to?

    <p>A strong electrostatic attraction between positive and negative ions.</p> Signup and view all the answers

    What color is observed when Cu2+ ions migrate towards the cathode?

    <p>Blue</p> Signup and view all the answers

    Solid ionic compounds are good conductors of electricity.

    <p>False</p> Signup and view all the answers

    What type of bond is formed when an empty orbital of one atom overlaps with a lone pair of another atom?

    <p>Dative covalent bond</p> Signup and view all the answers

    What happens to the layers of an ionic crystal when stress is applied?

    <p>The layers may slide over each other.</p> Signup and view all the answers

    Molecules with an overall dipole are termed non-polar.

    <p>False</p> Signup and view all the answers

    The ability of a positive ion to distort the electron density of a neighboring negative ion is called ______.

    <p>polarizing power</p> Signup and view all the answers

    Match the following terms with their correct definitions:

    <p>Polarizing power = Ability of a positive ion to distort a negative ion's electron cloud Polarisability = Ability of a negative ion to be distorted by a positive ion Expanded octet = The availability of d-subshell to accommodate extra electrons Simple molecule = Low melting and boiling points due to weak intermolecular forces</p> Signup and view all the answers

    What is the molecular formula for chloroethane?

    <p>C2H5Cl</p> Signup and view all the answers

    A free radical is a species that contains an unpaired electron and is __________.

    <p>uncharged</p> Signup and view all the answers

    Which of the following factors increases the polarizing power of a positive ion?

    <p>Higher charge</p> Signup and view all the answers

    Smaller sized ions produce weaker ionic bonds.

    <p>False</p> Signup and view all the answers

    Match the type of formula with its description:

    <p>Molecular Formula = Actual number of each atom in a molecule Empirical Formula = Simplest whole number ratio of atoms Structural Formula = Describes how atoms are joined together Displayed Formula = Shows every atom and bond in a molecule</p> Signup and view all the answers

    What characteristic of ionic compounds explains their high melting and boiling points?

    <p>Strong electrostatic attraction between oppositely charged ions in a giant lattice.</p> Signup and view all the answers

    Which of the following describes homolytic bond breaking?

    <p>Each bonding electron leaves with different atoms</p> Signup and view all the answers

    Geometric isomerism can occur in alkanes.

    <p>False</p> Signup and view all the answers

    Explain why free radical substitution has limited use in industry.

    <p>The yield is low due to further substitution reactions and separation of products.</p> Signup and view all the answers

    What happens to the atomic radius as you move down a group in the periodic table?

    <p>It increases</p> Signup and view all the answers

    The atomic radius decreases across each period due to increased nuclear charge.

    <p>True</p> Signup and view all the answers

    Define the term 'orbital'.

    <p>A region within an atom that can hold up to two electrons with opposing spins.</p> Signup and view all the answers

    Ionization energy is a measure of the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of __________.

    <p>gaseous ions</p> Signup and view all the answers

    Match the following elements with their electron configurations:

    <p>29Cu = 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10 24Cr = 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d Hydrogen = 1s1 Oxygen = 1s2, 2s2, 2p4</p> Signup and view all the answers

    Which factor primarily influences the ease of removing an outer electron as you move down a group?

    <p>Increased atomic radius</p> Signup and view all the answers

    Ionization energy generally decreases across a period.

    <p>False</p> Signup and view all the answers

    List the four main factors that affect ionization energy.

    <p>Nuclear charge, distance of outer electrons from the nucleus, shielding effect of inner electrons, spin-pair repulsion.</p> Signup and view all the answers

    What type of bond leads to restricted rotation in alkenes?

    <p>C=C double bond</p> Signup and view all the answers

    Secondary carbocations are less stable than primary carbocations.

    <p>False</p> Signup and view all the answers

    What is the term for the addition reaction involving an electrophile and an alkene?

    <p>Electrophilic addition</p> Signup and view all the answers

    Polymers are formed by the ________ of smaller molecules called monomers.

    <p>combination</p> Signup and view all the answers

    Match the following carbon structures to their properties:

    <p>Graphite = Conducts electricity Diamond = High melting point Benzene = Aromatic compound Carbon Black = Used in tires</p> Signup and view all the answers

    What is the primary disadvantage of recycling polymers?

    <p>Polymers need to be sorted and this is expensive.</p> Signup and view all the answers

    Electrophiles are species that are rich in electrons.

    <p>False</p> Signup and view all the answers

    What factor contributes to the higher ionization energy in elements with electrons removed from a lower main energy level?

    <p>Reduced electron-electron repulsion</p> Signup and view all the answers

    The difference in electronegativity between barium and chlorine is greater than that between ________ and chlorine.

    <p>beryllium</p> Signup and view all the answers

    Which properties of graphite allow it to conduct electricity?

    <p>Delocalized electrons</p> Signup and view all the answers

    Study Notes

    • Atomic radius decreases across each period due to increasing nuclear charge and similar shielding.
    • Atomic radius increases down each group due to increasing electron shells and decreasing attraction forces.

    Orbital Definitions

    • Orbital: a region within an atom that can hold up to two electrons with opposing spins.
    • Subshells: s (1 orbital), p (3 orbitals), d (5 orbitals)

    Quantum Shells

    • The first three quantum shells have 14 orbitals.

    Electron Configurations

    • Examples of electron configurations are provided (29Cu and 24Cr).

    Ionization Energy

    • Ionization energy: the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions.
    • Ionization energy increases across a period due to increasing nuclear charge and decreasing shielding.
    • Ionization energy decreases down a group due to increasing atomic radius and increasing shielding.

    Exceptions in Period 2

    • Boron's first ionization energy is less than beryllium's, despite having a greater nuclear charge, due to the outer electron being removed from a higher energy p orbital.
    • Oxygen's first ionization energy is less than nitrogen's due to increased electron-electron repulsion within the filled 2p orbitals in oxygen.

    Exceptions in Period 3

    • Aluminum's first ionization energy is less than magnesium's, despite having a greater nuclear charge, due to the outer electron being removed from a higher energy p orbital.
    • Sulfur's first ionization energy is less than phosphorus's due to increased electron-electron repulsion within the filled 3p orbitals.

    Polyatomic Ions

    • Provides a list of common polyatomic ions with their formulae and charges.

    Solubility Rules

    • Provides solubility rules for nitrates, sulfates, and halides that are an exception.

    Ionic Bonding

    • Ionic bond: strong electrostatic attraction between positive and negative ions, occurring in all directions.
    • High melting and boiling points due to strong attraction.
    • Bad conductors of electricity in solid state but good in molten and aqueous states.
    • Brittle due to repulsion between ions of same charge during stress.

    Polarisation

    • Polarisation: distortion of electron density in a negative ion (anion) by a positive ion (cation).
    • Polarising power: ability of cation to distort the electron density of the anion.
    • Factors which increase polarizing power: smaller size and higher charge of cation.

    Types of Covalent Bonds

    • Sigma bonds: formed by end-on overlap of orbitals, strong bonds.
    • Pi bonds: formed by sideways overlap of p orbitals, weaker bonds.

    Shapes of Molecules

    • Electron pair repulsion theory explains the shapes of molecules based on repulsion between bonding and lone pairs of electrons.
    • Different shapes are associated with different numbers of bonding and lone pairs (e.g., linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral).

    Bond Length and Strength

    • Bond length: distance between nuclei of bonded atoms.
    • Bond strength: energy required to break one mole of the bond in the gaseous state.
    • Shorter bonds have greater bond strength.

    Electronegativity

    • Electronegativity: ability of an atom to attract a bonding pair of electrons.
    • Decreases down the group due to increasing atomic radius and increasing shielding.
    • Inceases across a period

    Giant Covalent Structures

    • Allotropes of carbon (diamond, graphite, graphene) are examples of giant covalent structures.
    • Properties of each allotrope are provided in a tabular format (e.g., structure, melting and boiling points, conductivity, hardness).

    Metallic Bonding

    • Metallic bonding: strong electrostatic attraction between positive metal ions and delocalized electrons in a giant metallic lattice.
    • High melting and boiling points due to strong attraction.
    • Good conductors of electricity and heat due to free-moving delocalized electrons and the flow of kinetic energy.
    • Malleable and ductile due to the ability of the layers of positive ions to slide over another.

    Molecular and Empirical Formulae

    • Provides definitions and examples for both molecular and empirical formulae.

    Structural Formulae

    • Provides definition and examples for structural formulae.

    Addition Reactions

    • Addition reactions, of alkenes (and what they produce), the reagents used, and reaction conditions.

    Free Radicals

    • Free radical: a species with an unpaired electron and is uncharged.

    Isomers

    • Isomers: compounds with same molecular formula but different structures.
    • Geometric isomers (alkenes) are discussed.

    Alkenes

    • Alkenes have pi bonds which is a region of high electron density.
    • This makes the alkene molecule attractive to electrophiles.
    • Reactivity of alkenes is discussed (i.e. halogenation, oxidation).

    Mass Spectroscopy

    • Mass spectroscopy is a method used to analyze compounds. The data from a mass spectroscopy experiment determines the relative abundance of isotopes.
    • Isotopes in Chlorine are discussed.

    Incineration

    • Incineration advantages and disadvantages are provided.

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    Description

    This quiz covers key concepts of atomic radius trends, orbital definitions, quantum shells, electron configurations, and ionization energy. Understand how these concepts influence the properties of elements in the periodic table. Test your knowledge on exceptions in period 2 as well.

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