Atomic Structure Quiz
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Questions and Answers

What term describes the smallest constituent of matter?

  • Proton
  • Atom (correct)
  • Molecule
  • Nucleus

    • Which of the following particles has a negative electric charge?

  • Electron (correct)
  • Proton
  • Neutron
  • Nucleon

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

  • One
  • Two (correct)
  • Eight
  • Four

    • What is formed when an atom has more or fewer electrons than protons?

    <p>Ion (A)</p> Signup and view all the answers

    In the atomic structure, what constitutes the nucleus?

    <p>Protons and neutrons (A)</p> Signup and view all the answers

    Which term refers to electrons located in the outermost shell of an atom?

    <p>Valence electrons (C)</p> Signup and view all the answers

    Which of these particles is most associated with atomic mass?

    <p>Both protons and neutrons (D)</p> Signup and view all the answers

    How are orbitals grouped in the context of atomic structure?

    <p>By number (B)</p> Signup and view all the answers

    What is the molar mass of NaCl based on its constituent atomic masses?

    <p>58 g/mol (B)</p> Signup and view all the answers

    In a chemical reaction A + B → AB, which terms are considered reactants?

    <p>A and B (C)</p> Signup and view all the answers

    What is the molar mass of glucose (C6H12O6)?

    <p>180 g/mol (D)</p> Signup and view all the answers

    When calculating molar mass, which of the following elements would contribute 32 g/mol in O2?

    <p>2 Oxygen atoms (D)</p> Signup and view all the answers

    What does the chemical equation represent in a reaction?

    <p>The transformation of reactants into products (D)</p> Signup and view all the answers

    How is the molar mass of water (H2O) calculated?

    <p>(2×1) + (1×16) (A)</p> Signup and view all the answers

    What do chemists use to derive the atomic masses used in calculating molar mass?

    <p>Periodic table (B)</p> Signup and view all the answers

    Which type of elements tend to gain electrons and form anions?

    <p>Nonmetals (A)</p> Signup and view all the answers

    What defines the properties of metalloids?

    <p>They exhibit properties of both metals and nonmetals (B)</p> Signup and view all the answers

    Which group of elements is characterized as very reactive nonmetals often found as salts?

    <p>Halogens (D)</p> Signup and view all the answers

    Which element belongs to the alkali metals group?

    <p>Sodium (C)</p> Signup and view all the answers

    How do alkaline earth metals react with water compared to alkali metals?

    <p>They react fairly vigorously, but not as much as alkali metals (B)</p> Signup and view all the answers

    Which statement about noble gases is accurate?

    <p>They are generally unreactive and inert (A)</p> Signup and view all the answers

    What is a common property of nonmetals in solid state?

    <p>They are brittle (D)</p> Signup and view all the answers

    What percentage of elements in the periodic table are classified as metals?

    <p>75% (A)</p> Signup and view all the answers

    Which group includes elements that are known for their semiconductor properties?

    <p>Metalloids (A)</p> Signup and view all the answers

    What is the number of neutrons in a Cu atom?

    <p>36 (A)</p> Signup and view all the answers

    Which of the following describes a cation?

    <p>An atom with more protons than electrons (A)</p> Signup and view all the answers

    Which statement is correct regarding molecules?

    <p>Molecules are electrically neutral groups of atoms (D)</p> Signup and view all the answers

    How many protons are present in the isotope U-240?

    <p>92 (D)</p> Signup and view all the answers

    What is the charge of a magnesium ion (Mg2+)?

    <p>Positively charged (D)</p> Signup and view all the answers

    In the formation of F– ion, how many electrons does the fluorine atom gain?

    <p>1 (A)</p> Signup and view all the answers

    Which of the following best distinguishes ions from molecules?

    <p>Ions have distinct charges; molecules do not (B)</p> Signup and view all the answers

    Which option describes a property of anions?

    <p>They are negatively charged (D)</p> Signup and view all the answers

    What type of molecule is O2 considered?

    <p>Homonuclear (A)</p> Signup and view all the answers

    How would you classify the reaction Mg → Mg2+ + 2 e–?

    <p>Oxidation reaction (C)</p> Signup and view all the answers

    What is true about atoms of different elements?

    <p>They vary in size and mass. (C)</p> Signup and view all the answers

    Which statement correctly describes isotopes?

    <p>Isotopes of an element differ in mass number. (A)</p> Signup and view all the answers

    What does the atomic number represent?

    <p>The number of protons in the nucleus of an atom. (D)</p> Signup and view all the answers

    What characterizes a neutral atom?

    <p>It has equal numbers of protons and electrons. (A)</p> Signup and view all the answers

    How are isotopes identified?

    <p>By their mass numbers. (B)</p> Signup and view all the answers

    How can one differentiate between isotopes of carbon?

    <p>By their atomic mass. (B)</p> Signup and view all the answers

    What does a chemical reaction entail regarding atoms?

    <p>Rearrangement of existing atoms. (A)</p> Signup and view all the answers

    Which statement about elements and the periodic table is correct?

    <p>Elements have unique atomic numbers. (C)</p> Signup and view all the answers

    What defines a molecule in chemistry?

    <p>A simple whole-number ratio of combined elements. (C)</p> Signup and view all the answers

    Which of the following elements has 29 protons?

    <p>Copper (Cu) (A)</p> Signup and view all the answers

    Flashcards

    What is an Atom?

    The smallest unit of an element that can exist independently.

    What is the Nucleus?

    The central part of an atom, containing protons and neutrons.

    What are Protons?

    Positively charged particles found in the nucleus.

    What are Neutrons?

    Neutral particles found in the nucleus.

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    What are Electrons?

    Negatively charged particles that orbit the nucleus.

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    How are electrons arranged in an Atom?

    They are arranged in specific energy levels, called shells, around the nucleus. Each shell can hold a specific number of electrons.

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    What are Valence Electrons?

    Electrons in the outermost shell of an atom, involved in chemical bonding.

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    What is an Ion?

    An atom that has gained or lost electrons, resulting in a net positive or negative charge.

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    What defines an element?

    Atoms of the same element always have the same number of protons.

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    How are atoms different?

    Atoms of different elements have different numbers of protons.

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    Can one element change into another?

    Atoms of one element cannot change into atoms of another element through ordinary chemical reactions.

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    What is the atomic number?

    The number of protons in an atom's nucleus. It identifies the element.

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    What are isotopes?

    Atoms of the same element with the same number of protons but different numbers of neutrons.

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    What is the mass number?

    The total number of protons and neutrons in an atom's nucleus.

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    How do isotopes differ?

    Isotopes differ in their mass number due to varying numbers of neutrons.

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    What are the properties of isotopes?

    Isotopes of the same element have the same chemical properties but may differ in their physical properties.

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    What is the law of definite proportions?

    A simple whole-number ratio of the combined elements in a molecule.

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    What is a molecule?

    A molecule is a group of two or more atoms held together by chemical bonds, forming a neutral, electrically balanced unit.

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    What is a homonuclear molecule?

    A homonuclear molecule consists of atoms from the same element, like oxygen (O2).

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    What is a heteronuclear molecule?

    A heteronuclear molecule consists of atoms from different elements, like water (H2O).

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    What's a cation?

    Cations are formed when an atom loses one or more electrons, leading to a positive charge due to the excess of protons.

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    What's an anion?

    Anions are formed when an atom gains one or more electrons, leading to a negative charge due to the excess of electrons.

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    What type of elements form cations?

    Metal elements tend to form cations by losing electrons to achieve a more stable electron configuration.

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    What type of elements form anions?

    Non-metal elements tend to form anions by gaining electrons to achieve a more stable electron configuration.

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    What is a neutral species?

    A neutrally charged species with no overall charge, different from ions.

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    How is a molecule different from an ion?

    A molecule is distinguished from an ion by its lack of electrical charge.

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    Chemical Reaction

    A process that transforms one set of chemicals into another.

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    Chemical Equation

    A short way of describing a chemical reaction, using symbols and formulas.

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    Reactants

    The starting substances in a chemical reaction.

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    Products

    The substances formed during a chemical reaction.

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    How to calculate molar mass

    The molar mass of a substance is calculated by adding up the atomic masses of all the atoms in its chemical formula.

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    Relationship between atomic mass and molar mass

    The molar mass of an element in grams per mole (g/mol) is numerically equal to its atomic mass in atomic mass units (amu).

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    Importance of chemical formula for calculating molar mass

    To calculate the molar mass of any substance, you must know its exact chemical formula.

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    Nonmetals

    Elements located on the upper right side of the periodic table, characterized by poor conductivity of heat and electricity. They exist in all states of matter (solid, liquid, gas) and tend to gain electrons during chemical reactions, forming negatively charged ions (anions).

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    Metalloids

    Elements that lie along the zigzag line separating metals and nonmetals on the periodic table. They exhibit properties of both metals and nonmetals, are solid at room temperature, and are known as semiconductors due to their ability to conduct electricity under specific conditions. They are poor conductors of heat.

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    Alkali Metals

    Elements in Group 1A of the periodic table, highly reactive metals that readily lose electrons to form cations. They react violently with water, with sodium being a prime example.

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    Alkaline Earth Metals

    Elements in Group 2A of the periodic table, fairly reactive metals that are less reactive than alkali metals. They react with water, with calcium being a common example. Other members include magnesium, a lightweight structural metal.

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    Halogens

    Elements in Group 7A of the periodic table, highly reactive nonmetals that readily gain electrons to form anions. They are always found in salts. Examples include chlorine (a greenish-yellow gas), bromine (a red-brown liquid), iodine (a purple solid), and fluorine (a pale-yellow gas).

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    Noble Gases

    Elements in Group 8A of the periodic table, mostly unreactive (inert) gases. Helium, used in balloons, and neon, used in electronic signs, are well-known examples. Argon is a component of our atmosphere.

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    Electron affinity

    The tendency for elements to lose or gain electrons during chemical reactions.

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    Ionization

    The tendency for an atom to lose an electron and form a positive ion (cation). Metals have a high tendency for ionization.

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    Anions

    Negatively charged ions formed when an atom gains electrons.

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    Cations

    Positively charged ions formed when an atom loses electrons.

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    Study Notes

    Atomic Structure

    • Atoms are the smallest constituent of matter.
    • The word "atom" comes from the ancient Greek adjective "atomos," meaning "indivisible."
    • Atoms are divisible, consisting of a nucleus and surrounding electrons.
    • The nucleus is composed of protons and neutrons.
    • Protons have a positive electric charge and neutrons are electrically neutral.
    • Electrons have a negative electric charge.
    • The number of protons determines the identity of an element.
    • The number of protons (atomic number, Z) and neutrons (N) define the mass number (A).

    Nucleons

    • Protons and neutrons are collectively called nucleons.
    • More than 99.94% of an atom's mass is contained within the nucleus.

    Atomic Charge

    • If the number of protons and electrons are equal, the atom is electrically neutral.
    • If an atom has more or fewer electrons than protons, it's an ion with an overall net charge.

    Electrons in Atoms

    • Electrons are arranged in orbitals (s, p, d, and f).
    • An orbital holds a maximum of two electrons.
    • Orbitals are grouped into shells (1, 2, 3, and so on).

    Modern Atomic Theory and Laws

    • The theory that all matter is composed of atoms originated from several observations and laws.
    • The three primary laws are:
      • Law of conservation of mass
      • Law of definite proportions
      • Law of multiple proportions

    Law of Conservation of Mass

    • Matter is neither created nor destroyed in a chemical reaction.
    • The total mass of reactants equals the total mass of products.

    Law of Definite Proportions

    • A given chemical compound always contains the same elements in exactly the same proportions (by mass), regardless of its source or how it was prepared.

    Law of Multiple Proportions

    • When two elements "combine" to form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element are ratios of small whole numbers.

    Dalton's Atomic Theory

    • Each element is composed of tiny, indestructible particles called atoms.
    • An element's atoms are identical in size, mass, and properties.
    • Atoms of different elements vary in size and mass.
    • Atoms of one element cannot change into atoms of another element.
    • Atoms are indivisible and the chemical reaction leads to rearrangement of atoms not to their creation or destruction.
    • Molecules are simple whole-number ratios of combined elements.

    Elements: Defined by their Number of Protons

    • Each element has a unique name, symbol, and atomic number.
    • The symbol for an element usually consists of one or two letters.
    • Elements in the periodic table are arranged in order of increasing atomic number.

    Isotopes

    • Isotopes are atoms of one element that have the same number of protons (atomic number) and different numbers of neutrons.
    • Isotopes differ in mass number but are chemically identical.

    Molecules

    • Molecules are neutrally charged species that contain two or more atoms held together by chemical bonds.
    • Molecules are distinguished from ions by their lack of electrical charge.
    • A molecule may be homonuclear or heteronuclear.

    Ions: Charged Atoms

    • Cations form when an atom loses one or more electrons, and they carry a positive charge.
    • Anions form when an atom gains one or more electrons, and they carry a negative charge.

    Ions: Zwitter Ion

    • A Zwitter ion (also called a dipolar ion) is a neutral molecule that contains both positive and negative charges.

    The Modern Periodic Table

    • Arranged in order of increasing atomic number.
    • Organised into periods (rows) and groups (columns).
    • Similar physical and chemical properties within groups.

    Classification of Elements

    • Metals: Good conductors of heat and electricity, generally solids at room temperature, except mercury, often shiny.
    • Nonmetals: Poor conductors of heat and electricity, some are gases at room temperature.
    • Metalloids: Have properties of both metals and nonmetals (e.g. Semiconductors).

    Major Families

    • Alkali Metals (Group 1A): Highly reactive metals
    • Alkaline Earth Metals (Group 2A): Fairly reactive metals.
    • Halogens (Group 7A): Highly reactive nonmetals.
    • Noble Gases (Group 8A): Mostly unreactive (inert) gases.

    Chemical Formulas and Molecular Models

    • Compound: Distinct substance composed of two or more elements.
    • Chemical formula: Represents the type and number of each element in a molecule.

    Types of Different Formulas

    • Empirical formula: Simplest whole-number ratio of elements.
    • Molecular formula: Actual number of atoms of each element.
    • Structural formula: Diagram of how atoms are bonded together.

    Atomic Level View of Elements and Compounds

    • Atomic elements: Single atoms as particles (e.g., Fe, Na, Al).
    • Molecular elements: Multi-atom molecules (e.g., H₂, O₂, N₂).
    • Molecular compounds: Nonmetal atoms combined (e.g., H₂O, NH₃).
    • Ionic compounds: Metal and nonmetal atoms combined (e.g., NaCl).

    Molecular Elements

    • Certain elements exist as diatomic molecules (7 out of 118 elements in the periodic table): H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂.
    • Some other elements exist as polyatomic molecules (e.g., P₄, S₈, etc.).

    Chemical Reactions

    • A process that transforms one set of chemical substances into another.
    • Reactants are the initial substances involved; products are the resulting substances.
    • Chemical reactions are summarized by chemical equations.

    Chemical Equations

    • Chemical equations are shorthand representations of chemical reactions.
    • The equations include formulas for reactants and products, states (e.g., (g) for gas, (l) for liquid, (s) for solid, (aq) for aqueous) and sometimes energy symbols (e.g. heat).

    Balancing Chemical Equations

    • To show the reaction obeys the Law of Conservation of Mass, the equation must be balanced.
    • The number of each type of atom must be equal on both sides of the equation.

    Types of Chemical Equations

    • Molecular equations: Compounds are written as they exist (as molecules).
    • Ionic equations: Strong electrolytes are written as ions.
      • Net ionic equations: Show only the species involved in the reaction (leaving out spectator ions).

    Chemical Bonds

    • Compounds are formed from bonded atoms.
    • Chemical bonds are attractive forces between atoms.
    • Bonds arise from attraction between protons and electrons of bonded atoms.
    • Bonds can exist between atoms of the same element or between atoms of different elements.
    • Chemical bond formation lowers potential energy.

    Types of Chemical Bonds

    • Ionic bond: Transferring of electrons (metal-nonmetal)
    • Covalent bond: Sharing of electrons (nonmetal-nonmetal)
    • Metallic bond: Pooling of valence electrons

    Representing Valence Electrons with Dots (Lewis Structures)

    • Lewis structures are diagrams visualizing valence electrons using dots around an element's symbol.
    • Main-group element valence electrons equal its group number in the periodic table (except He).
    • Dots are placed singly around the symbol before pairing up (except He).

    Intermolecular Forces

    • Attractive forces between molecules.
    • Weaker than intramolecular forces (bonds).
    • Influence properties such as boiling point, melting point, solubility.
    • Types include London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

    Electronegativity and Bond Polarity

    • Electronegativity: Atom's ability to attract bonding electrons.
    • Higher for nonmetals, lower for metals.
    • Difference in electronegativity (ΔEN) affects bond polarity.
    • Polar bonds have partial charges (δ+ and δ-).

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