Atomic Structure and Periodic Table
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Questions and Answers

Which particles are negatively charged in an atom?

  • Nucleus
  • Protons
  • Electrons (correct)
  • Neutrons

    • Non-metals are located on the right side of the periodic table.

    True

    What determines an element's chemical behavior?

    the number of electrons in its atom, which in turn is determined by the number of protons.

    The nucleus of an atom is made up of protons and ________.

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

    Match the following types of elements with their characteristics:

    <p>Metals = Good conductors of heat and electricity Non-metals = Poor conductors Metalloids = Properties of both metals and non-metals</p> Signup and view all the answers

    What is the main difference between ionic bonds and covalent bonds?

    <p>Ionic bonds transfer electrons, while covalent bonds share electrons.</p> Signup and view all the answers

    Hydroxide (OH^-) is a polyatomic ion that carries a negative charge.

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

    What is the atomic symbol for Neon?

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

    Covalent bonds can be formed between two ___ elements.

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

    Match the following groups of the periodic table with their characteristics:

    <p>Alkali Metals = Highly reactive Noble Gases = Inert and non-reactive Halogens = Very reactive nonmetals Alkaline Earth Metals = Reactive metals but less than alkali metals</p> Signup and view all the answers

    What property of metals is influenced by the presence of delocalized electrons?

    <p>Electrical conductivity</p> Signup and view all the answers

    All elements are capable of forming covalent bonds.

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

    What do we call the electrons that are free to move in a metallic bond?

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

    What information does an electron dot diagram provide?

    <p>The number of electrons in the outer shell of an atom</p> Signup and view all the answers

    The first period of the periodic table can hold up to 8 elements.

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

    How many electrons can the second shell hold?

    <p>8</p> Signup and view all the answers

    All atoms in the same __________ have the same number of electrons in the outermost shell (__________ electrons).

    <p>group, valence</p> Signup and view all the answers

    All atoms in the same __________ have the same number of occupied __________ [__________].

    <p>period, shells, energy levels</p> Signup and view all the answers

    What will Oxygen's charge be when it becomes an ion?

    <p>-2</p> Signup and view all the answers

    Is it easier for Magnesium to gain or lose electrons?

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

    Match the following elements with the number of electrons they would ideally have in their outer shell:

    <p>Oxygen = 6 Magnesium = 2 Carbon = 4 Helium = 2</p> Signup and view all the answers

    What is the charge of the aluminium ion in aluminium oxide?

    <p>+3</p> Signup and view all the answers

    The total charge of the cations and anions in a crystal lattice must equal +1.

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

    How many sodium ions are needed to balance the charge of one nitride ion?

    <p>3</p> Signup and view all the answers

    In an ionic compound, magnesium must extbf{(gain/lose)} extbf{} electrons, while chloride must extbf{(gain/lose)} extbf{} electrons.

    <p>lose, gain</p> Signup and view all the answers

    Match the following ions with their respective charges:

    <p>Sodium = +1 Magnesium = +2 Chloride = -1 Oxide = -2</p> Signup and view all the answers

    What is the chemical name for NaCl?

    <p>Sodium Chloride</p> Signup and view all the answers

    The chemical formula for lead(II) iodide is PbI2.

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

    What is the formula for aluminum oxide?

    <p>Al2O3</p> Signup and view all the answers

    The chemical name for CaO is _____

    <p>Calcium Oxide</p> Signup and view all the answers

    Match the following ionic compounds with their chemical formulas:

    <p>Potassium Phosphate = K3P Barium Sulfide = BaS Copper(I) Bromide = CuBr Sodium Iodide = NaI</p> Signup and view all the answers

    Which of the following correctly identifies the ionic compound formed by copper(II) and sulfur?

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

    MgCl2 contains magnesium and oxygen.

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

    What is the cation in the ionic compound KI?

    <p>K^+</p> Signup and view all the answers

    Study Notes

    Atomic Structure

    • Elements are composed of atoms.
    • Atoms are made up of protons, neutrons, and electrons.
    • The nucleus of an atom contains protons and neutrons.
    • Electrons revolve around the nucleus in electron shells.
    • Protons are positively charged.
    • Neutrons have no charge.
    • Electrons are negatively charged.
    • Atoms have an overall neutral charge due to an equal number of protons and electrons.
    • The electrons in an atom determine its chemical behavior.
    • The atomic mass is determined by the sum of the number of protons and neutrons in the nucleus.

    The Periodic Table

    • The Periodic Table organizes elements based on their atomic structure.
    • The periods (horizontal rows) in the Periodic Table correspond to the number of electron shells filled in an atom.
    • The groups (vertical columns) in the Periodic Table represent elements with the same number of electrons in their outermost shell (valence electrons).
    • Electron dot diagrams depict the valence electrons of an atom surrounding its symbol.

    Electron Shell Configuration

    • Electron shell capacity: 2, 8, 8, 18, 18, 32, 32.
    • Atoms in the same period have the same number of electron shells.
    • Atoms in the same group have the same number of valence electrons.

    Forming Ions

    • Atoms strive to achieve a full outer shell.
    • Atoms can gain or lose electrons to achieve a stable electron configuration.
    • When an atom loses an electron, it becomes a positively charged ion (cation).
    • When an atom gains an electron, it becomes a negatively charged ion (anion).

    Ionic Bonding

    • Ionic bonding occurs between a metal and a non-metal.
    • The metal atom loses electrons, becoming a positively charged ion (cation).
    • The non-metal atom gains electrons, becoming a negatively charged ion (anion).
    • The opposite charges attract, creating an ionic bond.
    • Ionic compounds form crystal lattices, where cations and anions are arranged in a repeating pattern.
    • The total charge of the cations and anions in a crystal lattice must add up to zero.

    Naming Ionic Compounds

    • The name of the metal is written first, followed by the non-metal with the suffix "-ide" added.
    • Roman numerals are used to indicate the charge of transition metal ions.

    Covalent Bonding

    • Covalent bonding occurs between non-metal atoms.
    • Atoms share a pair of electrons to achieve a full outer shell.
    • The shared pair of electrons forms a covalent bond.

    Metallic Bonding

    • Occurs between metal atoms.
    • Metal atoms lose their valence electrons, creating a "sea" of delocalized electrons that move freely between the metal ions.
    • This "sea" of electrons accounts for the characteristic properties of metals:
      • Conductivity: The free movement of electrons allows metals to conduct electricity and heat.
      • Malleability: Metals can be hammered into thin sheets because the delocalized electrons provide flexibility.
      • Ductility: Metals can be drawn into wires because the delocalized electrons allow the metal ions to slide past each other.

    Notable Groups in the Periodic Table

    • Alkali Metals (Group 1): Highly reactive metals that react readily with water and oxygen.
    • Alkali Earth Metals (Group 2): Reactive metals, but less reactive than alkali metals.
    • Halogens (Group 17): Highly reactive non-metals that readily form ionic bonds with metals.
    • Noble Gases (Group 18): Unreactive gases that have a full outer shell of electrons.

    Year 8 Chem Revision - Elements, Compounds and Chemical Formula

    • Element: A pure substance that cannot be broken down into simpler substances.
    • Compound: A substance formed from two or more elements chemically combined in a fixed ratio.
    • Molecule: Two or more atoms joined together by covalent bonds.
    • Single atom: An isolated atom.
    • Lattice: A repeating arrangement of atoms or ions in a solid.
    • Chemical formula: Represents the elements and number of atoms present in a molecule or compound.
    • Subscripts in a chemical formula indicate the number of atoms of each element in the compound.
    • Example chemical formulas: O2, Ne, H2O, NaCl.
    • Metal: Generally shiny, malleable, and ductile, good conductors of heat and electricity.
    • Non-metal: Generally brittle, poor conductors of heat and electricity.
    • Metalloid: Shares properties of both metals and non-metals.

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    Year 9 Chemistry Booklet 2023 PDF

    Description

    Explore the fundamentals of atomic structure and the organization of elements in the Periodic Table. This quiz covers key concepts such as protons, neutrons, electrons, and how they determine an atom's properties. Test your understanding of electron configurations and the significance of valence electrons.

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