Atomic Structure Quiz
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Questions and Answers

What does the Pauli exclusion principle state regarding electrons in an orbital?

  • Each orbital must contain at least one electron before any can be paired.
  • Each orbital can contain any number of electrons regardless of their spin.
  • Each orbital may contain no more than two electrons with the same spin.
  • Each orbital can hold a maximum of two electrons with opposite spins. (correct)

    • According to Hund's rule, what is the preferred arrangement of electrons in p orbitals?

  • Electrons should fill the lower energy orbitals first regardless of the p sub-level.
  • Electrons can only occupy orbitals based on their spin state.
  • All electrons must pair up in the same orbital before occupying empty orbitals.
  • Electrons should occupy half of the empty orbitals before pairing in the same orbital. (correct)

    • How many electrons can a single p sub-level hold at maximum?

  • 4 electrons in two orbitals including pairing.
  • 8 electrons when considering all p orbitals.
  • 6 electrons across three orbitals. (correct)
  • 2 electrons in two separate orbitals.

    • What is the stability preference for electron arrangements in orbitals?

    <p>Electrons prefer to be alone in each orbital before pairing up.</p> Signup and view all the answers

    Which type of orbital exists in the first shell?

    <p>s orbital</p> Signup and view all the answers

    Why does the 4s orbital contain one electron in larger atoms?

    <p>The 3d sub-level being half-full or full is a more stable configuration.</p> Signup and view all the answers

    How many p orbitals are present in the second shell?

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

    Which of the following states the correct filling order of orbitals according to the Aufbau principle?

    <p>4s, 3d, 4p</p> Signup and view all the answers

    What shape does an s orbital have?

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

    What is the maximum number of electrons that an orbital can hold?

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

    Which of these rules states that each orbital must be filled singly before pairing?

    <p>Hund's rule</p> Signup and view all the answers

    Which of the following is true about the filling order of the third shell?

    <p>It contains s, p, and d orbitals.</p> Signup and view all the answers

    What is the principal quantum number associated with the f orbitals?

    <p>4</p> Signup and view all the answers

    What is the relative atomic mass of the sample of chlorine calculated in the content?

    <p>35.4</p> Signup and view all the answers

    What is the molar mass of sodium chloride (NaCl)?

    <p>58.5 g/mol</p> Signup and view all the answers

    How many moles are represented by 20 grams of a substance with a molar mass of 10 g/mol?

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

    Which of the following properties does NOT describe giant covalent substances?

    <p>Conduct electricity</p> Signup and view all the answers

    What is the characteristic structure of diamond?

    <p>Tetrahedral arrangement</p> Signup and view all the answers

    Which carbon allotrope has good electrical conductivity due to delocalised electrons?

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

    How many particles are in one mole as described by Avogadro’s number?

    <p>6.02 x 10^23</p> Signup and view all the answers

    Which of the following describes the bonding in giant covalent substances?

    <p>Strong covalent bonds</p> Signup and view all the answers

    What is the calculated number of moles in 2.842 g of sodium sulfate, Na2SO4?

    <p>0.0197</p> Signup and view all the answers

    How do you determine the empirical formula of a compound?

    <p>Divide all the moles by the smallest number</p> Signup and view all the answers

    What is the relative formula mass (RFM) of chlorine given 80% chlorine-35 and 20% chlorine-37?

    <p>35.4</p> Signup and view all the answers

    Given 828 g of lead and 64 g of oxygen, which of the following represents the empirical formula?

    <p>PbO2</p> Signup and view all the answers

    What is the primary reason for the malleability and ductility of metals?

    <p>Delocalised electrons allow layers to slide past each other.</p> Signup and view all the answers

    For a compound with a relative formula mass of 32 consisting of 87.5% nitrogen and 12.5% hydrogen, what is the empirical formula?

    <p>NH3</p> Signup and view all the answers

    Which of the following correctly describes covalent substances?

    <p>They may exist as solids, liquids, or gases at room temperature.</p> Signup and view all the answers

    Which statement about metallic bonding is true?

    <p>Metallic bonding results from the attraction between positive ions and delocalised electrons.</p> Signup and view all the answers

    Which step is NOT part of finding an empirical formula?

    <p>Calculating the total mass of the compound</p> Signup and view all the answers

    How many moles are present in 6.02 g of magnesium sulfate, MgSO4?

    <p>0.0501</p> Signup and view all the answers

    What is the relative atomic mass (Ar) of an element calculated from?

    <p>The sum of the isotopic masses multiplied by their abundances divided by total abundance.</p> Signup and view all the answers

    Which property of metallic substances is primarily due to delocalised electrons?

    <p>Good thermal conductivity.</p> Signup and view all the answers

    What is the first step in calculating the empirical formula for a sample of elements?

    <p>Find the moles of each atom</p> Signup and view all the answers

    Which combination of isotopic abundances is used to calculate the relative atomic mass of chlorine?

    <p>80% chlorine-35 and 20% chlorine-37.</p> Signup and view all the answers

    How do simple covalent substances differ from metallic bonding in their electrical conductivity?

    <p>Covalent substances do not conduct electricity at all.</p> Signup and view all the answers

    What structural feature characterizes a giant metallic lattice?

    <p>A 3D arrangement of positive ions and delocalised electrons.</p> Signup and view all the answers

    What does a saturated solution imply?

    <p>The maximum amount of solute has been dissolved.</p> Signup and view all the answers

    Which statement accurately describes a solute?

    <p>It can be solid, liquid, or gas in a solution.</p> Signup and view all the answers

    What represents the Law of Conservation of Mass in a chemical reaction?

    <p>The number of atoms before and after the reaction is equal.</p> Signup and view all the answers

    What does the coefficient in a balanced chemical equation indicate?

    <p>The number of molecules participating in the reaction.</p> Signup and view all the answers

    How is molarity calculated?

    <p>By dividing the number of moles of solute by the volume of solution in liters.</p> Signup and view all the answers

    What defines supersaturation in a solution?

    <p>A solution that has more solute than its solubility can hold at a given temperature.</p> Signup and view all the answers

    Which of the following is a characteristic of a reactant in a chemical equation?

    <p>It is a substance that changes during the reaction.</p> Signup and view all the answers

    In the empirical formula analysis, what does a subscript represent?

    <p>The number of atoms in a molecule.</p> Signup and view all the answers

    Study Notes

    Atomic Structure

    • Atoms are the smallest particles of chemical elements.
    • Elements are substances with atoms having the same number of protons (atomic number).
    • Protons are positively charged subatomic particles found in the atomic nucleus.
    • Neutrons are neutral subatomic particles also found in the atomic nucleus.
    • Electrons are negatively charged subatomic particles, much smaller than protons or neutrons.
    • The nucleus is the positively charged central core of an atom, containing protons and neutrons.
    • Almost all of an atom's mass is concentrated in its nucleus.
    • Atomic number is the number of protons in an atom's nucleus.
    • Isotopes are forms of the same element with the same number of protons but different numbers of neutrons, and therefore different masses.
    • Mass number is the total number of protons and neutrons in an atom's nucleus.
    • Relative atomic mass (Ar) is the ratio of the average mean mass of one atom of an element to one-twelfth the mass of an atom of carbon-12.

    Periodic Table

    • The order of elements in the periodic table is determined by their atomic number.
    • An element's position in the periodic table is also determined by its electronic structure, especially the outermost electron shell.
    • The number of electrons in the outermost shell determines the element's group.
    • The number of electron shells determines the period an element is in.

    Electronic Arrangement

    • Shells (energy levels) are described by a principal quantum number (n).
    • Each shell can hold up to 2n² electrons.
    • Different shells have different quantum numbers.
    • Electrons fill shells and sub-levels starting with the lowest energy levels first.
    • Sub-levels are s, p, d, and f.
    • Each sublevel holds a different maximum number of electrons (s = 2, p = 6, d = 10, f = 14).
    • Orbitals are regions within an atom that contain electrons having opposite spins.

    Electronic Configurations

    • The Aufbau principle describes how electrons fill atomic orbitals.
    • Electrons first fill the lowest energy levels.
    • Any orbital can hold a maximum of two electrons with opposite spins.

    Ionic Bonding

    • Involves the transfer of electrons between metal and non-metal atoms.
    • Metals lose electrons to form positive ions (cations).
    • Non-metals gain electrons to form negative ions (anions).
    • The electrostatic attraction between these oppositely charged ions forms the ionic bond.
    • lons are arranged in a crystal lattice structure.
    • lonic compounds are typically solid at room temperature and have high melting and boiling points.

    Covalent Bonding

    • Involves the sharing of electrons between non-metal atoms.
    • A covalent bond consists of a shared pair of electrons.
    • Covalent bonds are usually directional.
    • Properties of covalent bonds include low melting and boiling points, where covalent substances may exist as a solid, liquid or gas at room temperature.
    • Covalent compounds do not conduct electricity, as solids or liquids.
    • Dative covalent (coordinate) bonds are a type of covalent bond where both electrons in the shared pair come from the same atom.

    Metallic Bonding

    • Involves a lattice of positive metal ions surrounded by a "sea" of delocalised electrons.
    • Delocalised electrons are free to move throughout the lattice, giving rise to the electrical conductivity of metals.
    • The strong electrostatic attraction between the ions and delocalised electrons gives metals high melting and boiling points.
    • Metals are malleable and ductile, due to the layers of metal ions that can slide past one another.

    Mole Calculations

    • Relative molecular mass (Mr) is the sum of the atomic masses of all atoms in a molecule.
    • Moles (n) = mass (g) / Mr (g/mol).
    • Avogadro's constant is the number of atoms, molecules, or ions in one mole (6.02 x 10²³).

    Empirical Formula

    • The empirical formula is the simplest whole number ratio of atoms of each element in a compound.

    Percent Yield

    • Percentage Yield is a calculation that compares the amount of product made in a chemical reaction to the theoretical yield.

    Limiting Reagent

    • The limiting reagent is the reactant that determines the maximum amount of product that can be formed in a chemical reaction.

    Intermolecular Forces

    • London dispersion forces (temporary dipole-induced dipole forces) are weak intermolecular forces that act between all molecules, including nonpolar ones.
    • Dipole-dipole forces are stronger than London dispersion forces and act only between polar molecules.
    • Hydrogen bonds are a special type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine).

    Polar and Non-Polar Molecules

    • Polar molecules have a positive and negative end due to uneven electron distribution.
    • Non-polar molecules have an even distribution of electrons, resulting in no separation of charge.
    • Electronegativity is the tendency of an atom to attract bonding electrons to itself.

    Balancing Chemical Equations

    • Equations must follow the law of conservation of mass, stating that the number and type of atoms must remain the same on both sides of the equation.
    • Coefficients are used to balance chemical equations, modifying the number of molecules to ensure the quantity of each element is equal on both sides.

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    Chemistry Notes PDF

    Description

    Test your knowledge on the fundamental concepts of atomic structure, including the types of subatomic particles, atomic numbers, isotopes, and relative atomic mass. This quiz will help reinforce your understanding of how atoms are organized and their significance in the realm of chemistry.

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