Chemistry Chapter 5 - The Periodic Law
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Questions and Answers

In the modern periodic table, elements are ordered according to which of these?

  • According to Mendeleev's original design.
  • According to decreasing atomic mass.
  • Based on when they were discovered.
  • According to increasing atomic number. (correct)

    • Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing?

  • Atomic number
  • Atomic mass (correct)
  • Density
  • Reactivity

    • What does the modern periodic law state?

  • The chemical properties of elements can be grouped according to periodicity, but physical properties cannot.
  • Electrons exhibit properties of both particles and waves.
  • No two electrons with the same spin can be found in the same place in an atom.
  • The physical and chemical properties of an element are functions of its atomic number. (correct)

    • The discovery of the noble gases changed Mendeleev's periodic table by adding a new?

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

    The most distinctive property of the noble gases is that they are?

    <p>Largely unreactive</p> Signup and view all the answers

    Lithium, the first element in Group 1, has an atomic number of 3. The second element in this group has an atomic number of?

    <p>11</p> Signup and view all the answers

    An isotope of fluorine has a mass number of 19 and an atomic number of 9. How many protons are in this atom?

    <p>9</p> Signup and view all the answers

    An isotope of fluorine has a mass number of 19 and an atomic number of 9. How many neutrons are in this atom?

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

    A certain isotope contains 53 protons, 78 neutrons, and 54 electrons. What is its atomic number?

    <p>53</p> Signup and view all the answers

    A certain isotope contains 53 protons, 78 neutrons, and 54 electrons. What is the mass number of this atom?

    <p>131</p> Signup and view all the answers

    A certain isotope contains 53 protons, 78 neutrons, and 54 electrons. What is the name of this element?

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

    In a modern periodic table, every element is a member of both a horizontal row and a vertical column. Which one is the group, and which one is the period?

    <p>The group is the vertical column, and the period is the horizontal row.</p> Signup and view all the answers

    Explain the distinction between atomic mass and atomic number of an element.

    <p>The atomic number is the number of protons in an atom. The atomic mass is a weighted average of the masses of the naturally occurring isotopes of that element.</p> Signup and view all the answers

    There are 18 columns in the periodic table; each has a group number. Give the group numbers that make up each of the following blocks: s block, p block, d block.

    <p>1-2, 13-18, 3-12</p> Signup and view all the answers

    When an electron is added to a neutral atom, energy is?

    <p>Either absorbed or released</p> Signup and view all the answers

    The energy required to remove an electron from a neutral atom is the atom's?

    <p>Ionization energy</p> Signup and view all the answers

    From left to right across a period on the periodic table, electron affinity values tend to become more?

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

    From left to right across a period on the periodic table, ionization energy values tend to?

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

    From left to right across a period on the periodic table, atomic radii tend to become?

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

    Name the halogen with the least-negative electron affinity.

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

    Name the alkali metal with the highest ionization energy.

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

    Name the element in Period 3 with the smallest atomic radius.

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

    Name the Group 14 element with the largest electronegativity.

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

    Compare the radius of a positive ion to the radius of its neutral atom.

    <p>The radius of a positive ion is smaller than the radius of its corresponding neutral atom.</p> Signup and view all the answers

    Compare the radius of a negative ion to the radius of its neutral atom.

    <p>The radius of a negative ion is larger than the radius of its corresponding neutral atom.</p> Signup and view all the answers

    Give the approximate positions and blocks where metals and nonmetals are found in the periodic table.

    <p>Metals are on the left side of the periodic table, mostly in the s, d, and f blocks. Nonmetals are on the right side of the periodic table, all in the p block (except for hydrogen).</p> Signup and view all the answers

    Of metals and nonmetals, which tend to form positive ions? Which tend to form negative ions?

    <p>Metals tend to form positive ions; nonmetals tend to form negative ions.</p> Signup and view all the answers

    Explain why the second ionization energy is higher than the first, the third is higher than the second, and so on.

    <p>As electrons are removed in successive ionizations, fewer electrons remain within the atom to shield the attractive force of the nucleus. Each electron removed from an ion experiences a stronger effective nuclear pull than the electron removed before it.</p> Signup and view all the answers

    Explain the role of valence electrons in the formation of chemical compounds.

    <p>Valence electrons are the electrons most subject to the influence of nearby atoms or ions. They are the electrons available to be lost, gained, or shared in the formation of chemical compounds.</p> Signup and view all the answers

    Consider the neutral atom with 53 protons and 74 neutrons to answer the following questions. a. What is its atomic number? b. What is its mass number? c. Is the element's position in a modern periodic table determined by its atomic number or by its atomic mass?

    <p>53, 127, atomic number</p> Signup and view all the answers

    Consider an element whose outermost electron configuration is 3d10 4s2 4p x. a. To which period does the element belong? b. If it is a halogen, what is the value of x? c. The group number will equal (10 + 2 + x). True or False?

    <p>Period 4, 5, true</p> Signup and view all the answers

    A. In which block are metalloids found, s, p, d, or f? b. In which block are the hardest, densest metals found, s, p, or d?

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

    Name the most chemically active halogen.

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

    Which class has greater ionization energies, metals or nonmetals?

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

    An element with a large negative electron affinity is most likely to form a?

    <p>Negative ion</p> Signup and view all the answers

    In general, which has a stronger electron attraction, a large atom or a small atom?

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

    Who was credited with developing a method that led to the determination of standard relative atomic masses?

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

    Who created a table in which elements with similar properties were grouped together, and discovered the periodic law?

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

    Who discovered that the elements fit into patterns better when they were arranged according to atomic number rather than atomic weight and established atomic numbers?

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

    This states that the physical and chemical properties of the elements are periodic functions of their atomic numbers?

    <p>The periodic law</p> Signup and view all the answers

    What is an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column or group?

    <p>Modern periodic table</p> Signup and view all the answers

    Name three sets of elements that have been added to the periodic table since Mendeleev's time.

    <p>Noble gases, lanthanides, actinides</p> Signup and view all the answers

    The length of a period is determined by...?

    <p>The number of electrons that can occupy sub-levels being filled in that period.</p> Signup and view all the answers

    What are the 4 blocks?

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

    Noble gases are __________ in relation to reactivity.

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

    Group 1 elements, otherwise known as the ________ _________ are silvery and soft enough to cut with a knife?

    <p>Alkali metals</p> Signup and view all the answers

    Alkali metals are ___________ in relation to reactivity?

    <p>Very reactive</p> Signup and view all the answers

    Group 2 elements, otherwise known as _______ ________ _________ are less reactive, but still too reactive to be found in pure form?

    <p>Alkaline earth metals</p> Signup and view all the answers

    The d - block elements are metals with typical metallic properties and are often referred to as what?

    <p>Transition metals</p> Signup and view all the answers

    Groups 13-18 are the ___ block.

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

    Group 17 elements are the _________

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

    The p-block elements together with the s - block elements are called the what?

    <p>Main-group elements</p> Signup and view all the answers

    What are the most reactive nonmetals?

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

    What are wedged between Groups 3 and 4 in the sixth and seventh periods?

    <p>F-block elements</p> Signup and view all the answers

    The first row of f-block are?

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

    The second row of f-block are?

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

    Actinides are very __________.

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

    What are the group 18 elements?

    <p>Noble gases</p> Signup and view all the answers

    What is half the distance between the nuclei of identical atoms that are bonded together?

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

    The farther to the right atomic radii are found across a period, the _________ the atom. This is caused by an increasing positive charge of the nucleus, which...?

    <p>Smaller, attracts electrons toward the nucleus.</p> Signup and view all the answers

    The atomic radii of the main-group elements ______________ down a group.

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

    An atom or group of bonded atoms that has a positive or negative charge.

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

    Any process that results in the formation of an ion.

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

    The energy required to remove one electron from a neutral atom of an element is the...?

    <p>Ionization energy</p> Signup and view all the answers

    Ionization energy ______ across a period, and __________ down a group.

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

    Each successive electron removed from an ion feels...?

    <p>An increasingly stronger effective nuclear charge</p> Signup and view all the answers

    The energy change that occurs when an electron is acquired by a neutral atom is called the atom's...

    <p>Electron affinity</p> Signup and view all the answers

    Electron affinity generally __________ across a period, _________ down a group.

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

    A positive ion is known as a...

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

    A negative ion is known as a...

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

    Formation of a cation by the loss of one or more electrons always leads to a ___________ in atomic radius?

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

    Formation of an anion by the addition of one or more electrons always leads to an ____________ in atomic radius?

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

    There is a gradual increase of ionic radii where?

    <p>Down a group</p> Signup and view all the answers

    The electrons available to be lost, gained, or shared in the formation of chemical compounds are referred to as the what?

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

    A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

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

    In the p-block, you calculate the number of valence electrons by doing what?

    <p>Group number - 10</p> Signup and view all the answers

    Electronegativities tend to __________ across each period.

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

    Study Notes

    The Periodic Law and Atomic Structure

    • Modern periodic table organizes elements by increasing atomic number.
    • Mendeleev observed similarities in chemical properties at regular intervals in terms of atomic mass.
    • Modern periodic law states element properties are functions of atomic number, not atomic mass.

    Noble Gases and Element Groups

    • Discovery of noble gases added a new group to Mendeleev’s periodic table.
    • Noble gases, found in Group 18, are characterized by low reactivity.
    • Alkali metals (Group 1) are silvery, soft, and very reactive; alkaline earth metals (Group 2) are less reactive.

    Atomic Structure and Isotopes

    • Isotopes are defined by mass number (protons + neutrons) and atomic number (protons).
    • Atomic number determines element identity; for fluorine, mass number is 19, atomic number is 9.

    Periods, Groups, and Blocks in the Periodic Table

    • Elements belong to periods (horizontal rows) and groups (vertical columns) based on properties.
    • Different blocks: s (Groups 1-2), p (Groups 13-18), d (Groups 3-12), f (lanthanides and actinides).

    Ionization Energy and Electron Affinity

    • Ionization energy requires energy to remove electrons; it increases across a period and decreases down a group.
    • Electron affinity measures the energy change when an electron is gained; it increases across a period and decreases down a group.

    Atomic and Ionic Radii

    • Atomic radii decrease across a period due to increased nuclear charge attracting electrons closer.
    • Positive ions (cations) have smaller radii than their neutral atoms; negative ions (anions) have larger radii.

    Valence Electrons and Chemical Reactivity

    • Valence electrons define an atom’s ability to form bonds, lost or gained during chemical reactions.
    • Electronegativity, the ability of an atom to attract electrons, tends to increase across a period.

    Reactivity of Halogens and Nonmetals

    • Halogens (Group 17) are highly reactive nonmetals, with fluorine being the most reactive.
    • Nonmetals typically form negative ions while metals form positive ions.

    Historical Figures and Contributions

    • Cannizzaro developed methods for standard atomic masses.
    • Mendeleev created tables grouping elements by properties and discovering periodic law.
    • Moseley determined elements fit better by atomic number rather than atomic weight.
    • Ionization energy increases with successive electron removal because of stronger effective nuclear charge.
    • The radius of positive ions is smaller; negative ions have a larger radius compared to their neutral counterparts.
    • Group 14 elements have varying electronegativities, with patterns observable in different periods and blocks of elements.

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    Test your knowledge of Chapter 5 on The Periodic Law with these flashcards. This quiz covers key concepts such as the arrangement of elements in the periodic table and the observations made by Mendeleev. Challenge yourself to recall essential definitions and properties of elements.

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