Chemistry Unit IV-VI Quiz
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Questions and Answers

What is the expected electron configuration for Copper (Cu)?

  • [Ar] 4s13d10
  • [Ar] 4s23d9 (correct)
  • [Ar] 4s24d9
  • [Ar] 4s23d8

    • What does Hund's Rule state?

  • Electrons occupy orbitals in pairs before any orbital is singly occupied.
  • Every orbital is singly occupied before any orbital gets doubly occupied. (correct)
  • All orbitals of the same energy must have one electron before any can have two.
  • Electrons fill the lowest available energy levels first.

    • Electromagnetic waves are classified only based on their energy levels.

    False

    What happens to an electron when it absorbs light?

    <p>It becomes excited and jumps to a higher energy level.</p> Signup and view all the answers

    The distance between two successive peaks of a wave is known as its ______.

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

    What is the electron configuration for sodium using the shorthand method?

    <p>[Ne] 3s1</p> Signup and view all the answers

    The shorthand electron configuration can be used for period 1 elements.

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

    Elements in family 7A typically gain 1 electron to achieve stability.

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

    An element must attain _____ valence electrons to be stable per the octet rule.

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

    Which of the following elements follows the duplet rule instead of the octet rule?

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

    Match the family of elements with their valence electron count:

    <p>1A = 1 2A = 2 6A = 6 8A = 8</p> Signup and view all the answers

    Match the following types of electromagnetic radiation with their characteristics:

    <p>Gamma-ray = Highest frequency and energy Radio waves = Lowest frequency and energy Visible Light = Colors range from violet to red X-ray = Used for medical imaging</p> Signup and view all the answers

    When an atom loses an electron, it gains a _____ charge.

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

    How many periods are there in the periodic table?

    <p>7</p> Signup and view all the answers

    Family A consists only of transition metals.

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

    What is the maximum number of electrons that can occupy an 's' orbital?

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

    The ______ state occurs when all energy levels in an atom are full.

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

    Match the following types of orbitals with their maximum electron capacity:

    <p>s = 2 electrons p = 6 electrons d = 10 electrons f = 14 electrons</p> Signup and view all the answers

    Which group is known as the Noble Gases?

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

    According to the Pauli exclusion principle, two electrons in the same orbital must have the same spin.

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

    What principle states that electrons fill the lowest available energy subshells first?

    <p>Aufbau principle</p> Signup and view all the answers

    What is the electron configuration of Yttrium (39)?

    <p>1s22s22p63s23p64s2 3d10 4p6 5s2 4d1</p> Signup and view all the answers

    Yttrium belongs to Group 2B.

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

    How many valence electrons does Yttrium have?

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

    Yttrium is located in Period __.

    <p>5</p> Signup and view all the answers

    What is the number of d-orbital electrons in Yttrium?

    <p>1</p> Signup and view all the answers

    Match the following properties to their values for Yttrium:

    <p>Electron configuration = 1s22s22p63s23p64s2 3d10 4p6 5s2 4d1 Group = 3B Valence electrons = 3 Period = 5</p> Signup and view all the answers

    The energy level of Yttrium is determined by its group number.

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

    What is the rule to find the Group number for Yttrium?

    <p>Add 2 to the number of d-orbital electrons.</p> Signup and view all the answers

    Which element has the largest atomic radius?

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

    The ionic size increases from left to right across a period.

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

    Define ionization energy.

    <p>The energy needed to remove an electron from an atom.</p> Signup and view all the answers

    The distance from the nucleus of a neutral atom to the outermost shell is called the atomic __________.

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

    Match the following ions with their expected size relationship:

    <p>Na+ = Smaller than Na Mg2+ = Smaller than Na+ Cl- = Bigger than Na+ Fe2+ = Smaller than Fe</p> Signup and view all the answers

    What happens to atomic radius as you move from top to bottom in a group?

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

    Anions are always larger than their corresponding neutral atoms.

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

    When an atom loses electrons, its ionic size __________.

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

    Which of the following statements is correct regarding nonmetals?

    <p>Nonmetals are good insulators.</p> Signup and view all the answers

    The atomic size increases from left to right across the periodic table.

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

    What is the charge of a nitride ion?

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

    The formula for sulfate ion is ______.

    <p>SO4^2-</p> Signup and view all the answers

    Match the following ions with their corresponding formulas:

    <p>Ammonium = NH4+ Phosphate = PO4^3- Sulfite = SO3^2- Chloride = Cl-</p> Signup and view all the answers

    Which element has the highest electronegativity?

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

    The ionization energy increases as you move down a group in the periodic table.

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

    What type of compound is formed when a cation pairs with an anion?

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

    A binary ionic compound is composed of ______ elements.

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

    Which property of metals increases from top to bottom in the periodic table?

    <p>Metallic properties</p> Signup and view all the answers

    What is the possible range of values for the electron spin quantum number (ms)?

    <p>+½, -½</p> Signup and view all the answers

    An electron with a spin quantum number of -½ is said to be spinning in a clockwise direction.

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

    What does a positive value of the electron spin quantum number (ms) indicate about the electron's spin?

    <p>upward spin</p> Signup and view all the answers

    The periodic law states that the physical and chemical properties of an element tend to vary periodically in order of increasing _______.

    <p>atomic number</p> Signup and view all the answers

    Match the following electron configurations with their corresponding electron spin states:

    <p>3s1 = +½ 3p4 = -½ 4d5 = +½ 3p3 = +½</p> Signup and view all the answers

    Which scientist is known as the Father of the Periodic Table?

    <p>Dmitri Mendeleev</p> Signup and view all the answers

    Henry Moseley arranged elements by their atomic mass.

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

    What did John Newlands contribute to the development of the periodic table?

    <p>Law of Octaves</p> Signup and view all the answers

    The average of the atomic masses of the first and third elements in Döbereiner's triads is equal to the atomic mass of the ______ element.

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

    Match each scientist with their contribution to the periodic table:

    <p>Johann Wolfgang Döbereiner = Law of Triads John Newlands = Law of Octaves Dmitri Mendeleev = First Periodic Table Henry Moseley = Periodic Table Law</p> Signup and view all the answers

    What major change did Moseley make to the arrangement of the periodic table?

    <p>Arranged by atomic number</p> Signup and view all the answers

    Döbereiner’s Law of Triads is based on the atomic number of elements.

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

    The periodic table is a tabular arrangement of chemical elements organized according to increasing ______.

    <p>atomic number</p> Signup and view all the answers

    Which electron configuration corresponds to the element with 8 valence electrons in Group 8A and Period 2?

    <p>1s2 2s2 2p6</p> Signup and view all the answers

    The maximum number of electrons that can occupy a p orbital is 8.

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

    Identify the element that has the electron configuration 1s2 2s2 2p6.

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

    In period 2, family 8A, the total number of electrons is _____.

    <p>10</p> Signup and view all the answers

    Match the following elements with their corresponding group and period:

    <p>Magnesium = 2A, 3 Hydrogen = 1, 1 Neon = 8A, 2 Oxygen = 6A, 2</p> Signup and view all the answers

    What happens to ionization energy as you move from left to right across a period?

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

    Electron affinity increases from top to bottom in a group.

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

    What is electronegativity?

    <p>The ability of an atom to attract electrons and gain a negative charge.</p> Signup and view all the answers

    Ionization energy is opposite the atomic _____

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

    Match the following trends with their descriptions:

    <p>Ionization Energy = Increases from left to right Electron Affinity = Increases from left to right Electronegativity = Increases from left to right Atomic Radius = Decreases from left to right</p> Signup and view all the answers

    Which of the following statements about ionization energy is correct?

    <p>It requires more energy to remove an electron from an atom with 8 valence electrons.</p> Signup and view all the answers

    Higher electronegativity means an atom is more likely to lose electrons.

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

    Explain why it is easier for atoms on the left side of the periodic table to lose electrons.

    <p>Atoms on the left have fewer valence electrons and less nuclear attraction, making it easier to lose them.</p> Signup and view all the answers

    The Aufbau principle states that electrons fill the highest energy subshells first.

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

    How many groups (families) are present in the periodic table?

    <p>18</p> Signup and view all the answers

    The group of elements known as ______ gases is found in family 8A.

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

    Match the following groups of elements with their corresponding names:

    <p>1A = Alkali Metals 2A = Alkaline Earth Metals 7A = Halogens 8A = Noble Gases</p> Signup and view all the answers

    Which of the following best describes an excited state of an atom?

    <p>Electrons jump to higher energy levels</p> Signup and view all the answers

    Which principle states that a maximum of two electrons may occupy an orbital if they have opposite spins?

    <p>Pauli exclusion principle</p> Signup and view all the answers

    What is the primary factor that determines the charge of an element in family 1A?

    <p>The ease of losing one electron</p> Signup and view all the answers

    The valence electrons for noble gases like neon are considered when determining their stability.

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

    For an atom to be stable, it must follow the octet rule, which states that an element must attain _____ valence electrons.

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

    Match the elements to their corresponding group number based on valence electrons:

    <p>Hydrogen = 1A Beryllium = 2A Aluminum = 3A Oxygen = 6A</p> Signup and view all the answers

    According to Hund’s Rule, how should electrons be filled in the orbitals?

    <p>Each orbital must have one electron before any has two</p> Signup and view all the answers

    The electron configuration 1s22s22p6 is equivalent to the configuration of Argon.

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

    In family 6A, the charge of elements is typically _____ when they attain stability.

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

    Study Notes

    Chemistry Study Notes

    • Q1 9-CONCHEM: This likely refers to a specific unit or chapter in a Chemistry course, within the first quarter
    • Q2 9-CONCHEM: Similar to Q1, this likely refers to a chemistry unit or chapter in the second quarter of the semester
    • UNIT IV: Order Among Elements: This unit covers the development and organization of the periodic table, including chemical symbols, electron configuration, group numbers, valence electrons, and trends in the periodic table
    • UNIT V: Stoichiometry: This unit discusses calculations related to chemical reactions, including chemical formulas, mole concept, molar mass, percentage composition, empirical and molecular formulas, balancing chemical equations, types of chemical reactions, and calculations based on balanced equations
    • UNIT VI: Chemical Bond: This section covers types of chemical bonds (ionic, covalent, metallic), octet rule, Lewis symbols, bond polarity, electronegativity, molecular geometry and intermolecular forces
    • 4.1-3 The Periodic Table: This section of the notes explains how the periodic table is organized and arranged and includes the historical development of the periodic table
    • 1817: Johann Wolfgang Döbereiner's Law of Triads: Döbereiner grouped elements into sets of three exhibiting similar properties. The average of the atomic mass of the first and third element approximates the second element's atomic weight
    • 1865: John Newlands's Law of Octaves: Newlands arranged elements based on increasing atomic mass. Elements with similar properties recurred every eighth element (like an octave in music) (applicable to elements before Calcium).
    • 1869: Dmitri Mendeleev's Periodic Table: Mendeleev's table organized by increasing atomic number. It contained spaces for undiscovered elements
    • 1913: Henry Moseley's Periodic Table: This modern periodic table is organized by atomic number, not atomic mass, leading to a more accurate arrangement.
    • 4.4 Electron Configuration: Explains the distribution of electrons in atomic orbitals, including ground and excited states, and the principles of Aufbau, Hund's rule, and Pauli exclusion to determine the electron configuration
    • 4.5 Valence Electrons and Blocks: This explains valence electrons (electrons in the outermost shell), the octet rule, how to relate valence electrons to the group number, and how they are organized in blocks in the periodic table
    • 4.6 Electromagnetic Radiation and Quantum Numbers: This section covers the structure and properties of electromagnetic waves, the full electromagnetic spectrum, and relationships among energy, wavelength, frequency to understand quantum behavior and properties
    • 4.7 Periodic Trends: This unit addresses how atomic properties like atomic size, ionization energy, electron affinity, electronegativity, metallic, and non-metallic properties change across a period and down a group.
    • UNIT V: Stoichiometry - Monatomic lons: Provides a table for monatomic ions and their charges (e.g. Li+, Na+, Mg2+, Al3+, etc.)
    • UNIT V: Stoichiometry - Polyatomic Ions: Provides a table for polyatomic ions and their formulas (e.g. nitrate, sulfate, phosphate, hydroxide, carbonate, etc.)
    • 5.1 Naming and Writing lonic Formulas: Explains the naming and writing of formulas for ionic compounds. Discusses the relationship between the charge of ions and the formulas of ionic compounds.
    • 5.3 Balancing Chemical Equations: Explains chemical equations, how to balance chemical equations by adjusting coefficients to maintain the law of conservation of mass (the number of atoms of each element must be the same on both sides of the equation).
    • Q3 9-CONCHEM, Q4 9-CONCHEM: These denote third and fourth quarter units or chapters in the 9-CONCHEM course, respectively.

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