Chapter 6 Practice Test

Chapter 6 Practice Test

Matching

Match each item with the correct statement below.

a. / electronegativity / f. / periodic law
b. / ionization energy / g. / cation
c. / atomic radius / h. / period
d. / metal / i. / group
e. / transition metal / j. / electrons

____1.horizontal row in the periodic table

____2.vertical column in the periodic table

____3.A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____4.type of element that is a good conductor of heat and electric current

____5.type of element characterized by the presence of electrons in the d orbital

____6.one-half the distance between the nuclei of two atoms when the atoms are joined

____7.type of ion formed by Group 2A elements

____8.subatomic particles that are transferred to form positive and negative ions

____9.ability of an atom to attract electrons when the atom is in a compound

____10.energy required to remove an electron from an atom

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____11.What is another name for the representative elements?

a. / Group A elements / c. / Group C elements
b. / Group B elements / d. / transition elements

____12.What is another name for the transition metals?

a. / noble gases / c. / Group B elements
b. / Group A elements / d. / Group C elements

____13.Which of the following elements is in the same period as phosphorus?

a. / carbon / c. / nitrogen
b. / magnesium / d. / oxygen

____14.Each period in the periodic table corresponds to ____.

a. / a principal energy level / c. / an orbital
b. / an energy sublevel / d. / a suborbital

____15.The modern periodic table is arranged in order of increasing atomic ____.

a. / mass / c. / number
b. / charge / d. / radius

____16.Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?

a. / Henry Moseley / c. / John Dalton
b. / Antoine Lavoisier / d. / Dmitri Mendeleev

____17.Which of the following categories includes the majority of the elements?

a. / metalloids / c. / metals
b. / liquids / d. / nonmetals

____18.Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a. / Pt / c. / Li
b. / V / d. / Kr

____19.To what category of elements does an element belong if it is a poor conductor of electricity?

a. / transition elements / c. / nonmetals
b. / metalloids / d. / metals

____20.In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a. / In, 49 protons, 49 electrons / c. / Cs, 55 protons, 132.9 electrons
b. / Zn, 30 protons, 60 electrons / d. / F, 19 protons, 19 electrons

____21.The atomic number of an element is the total number of which particles in the nucleus?

a. / neutrons / c. / electrons
b. / protons / d. / protons and electrons

____22.What element has the electron configuration 1s2s2p3s3p?

a. / nitrogen / c. / silicon
b. / selenium / d. / silver

____23.Which of the following is true about the electron configurations of the noble gases?

a. / The highest occupied s and p sublevels are completely filled.
b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.

____24.Elements that are characterized by the filling of p orbitals are classified as ____.

a. / groups 3A through 8A / c. / inner transition metals
b. / transition metals / d. / groups 1A and 2A

____25.Which of the following electron configurations is most likely to result in an element that is relatively inactive?

a. / a half-filled energy sublevel
b. / a filled energy sublevel
c. / one empty and one filled energy sublevel
d. / a filled highest occupied principal energy level

____26.Which subatomic particle plays the greatest part in determining the properties of an element?

a. / proton / c. / neutron
b. / electron / d. / none of the above

____27.Which of the following elements is a transition metal?

a. / cesium / c. / tellurium
b. / copper / d. / tin

____28.Which of the following groupings contains only representative elements?

a. / Cu, Co, Cd / c. / Al, Mg, Li
b. / Ni, Fe, Zn / d. / Hg, Cr, Ag

____29.Which of the following is true about the electron configurations of the representative elements?

a. / The highest occupied s and p sublevels are completely filled.
b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.

____30.What are the Group 1A and Group 7A elements examples of?

a. / representative elements / c. / noble gases
b. / transition elements / d. / nonmetallic elements

____31.Of the elements Fe, Hg, U, and Te, which is a representative element?

a. / Fe / c. / U
b. / Hg / d. / Te

____32.How does atomic radius change from top to bottom in a group in the periodic table?

a. / It tends to decrease. / c. / It first increases, then decreases.
b. / It tends to increase. / d. / It first decreases, then increases.

____33.How does atomic radius change from left to right across a period in the periodic table?

a. / It tends to decrease. / c. / It first increases, then decreases.
b. / It tends to increase. / d. / It first decreases, then increases.

____34.What causes the shielding effect to remain constant across a period?

a. / Electrons are added to the same principal energy level.
b. / Electrons are added to different principal energy levels.
c. / The charge on the nucleus is constant.
d. / The atomic radius increases.

____35.Atomic size generally ____.

a. / increases as you move from left to right across a period
b. / decreases as you move from top to bottom within a group
c. / remains constant within a period
d. / decreases as you move from left to right across a period

____36.What element in the second period has the largest atomic radius?

a. / carbon / c. / potassium
b. / lithium / d. / neon

____37.Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?

a. / more shielding of the electrons by the highest occupied energy level
b. / an increase in size of the nucleus
c. / an increase in number of protons
d. / fewer electrons in the highest occupied energy level

____38.Which of the following elements has the smallest atomic radius?

a. / sulfur / c. / selenium
b. / chlorine / d. / bromine

____39.What is the charge of a cation?

a. / a positive charge
b. / no charge
c. / a negative charge
d. / The charge depends on the size of the nucleus.

____40.Which of the following statements is true about ions?

a. / Cations form when an atom gains electrons.
b. / Cations form when an atom loses electrons.
c. / Anions form when an atom gains protons.
d. / Anions form when an atom loses protons.

____41.The metals in Groups 1A, 2A, and 3A ____.

a. / gain electrons when they form ions / c. / all have ions with a 1 charge
b. / all form ions with a negative charge / d. / lose electrons when they form ions

____42.Which of the following statements is NOT true about ions?

a. / Cations are positively charged ions.
b. / Anions are common among nonmetals.
c. / Charges for ions are written as numbers followed by a plus or minus sign.
d. / When a cation forms, more electrons are transferred to it.

____43.Why is the second ionization energy greater than the first ionization energy?

a. / It is more difficult to remove a second electron from an atom.
b. / The size of atoms increases down a group.
c. / The size of anions decreases across a period.
d. / The nuclear attraction from protons in the nucleus decreases.

____44.In which of the following sets are the charges given correctly for all the ions?

a. / Na, Mg, Al / c. / Rb, Ba, P
b. / K, Sr, O / d. / N, O, F

____45.In which of the following groups of ions are the charges all shown correctly?

a. / Li, O, S / c. / K, F, Mg
b. / Ca, Al, Br / d. / Na, I, Rb

____46.What is the element with the lowest electronegativity value?

a. / cesium / c. / calcium
b. / helium / d. / fluorine

____47.What is the element with the highest electronegativity value?

a. / cesium / c. / calcium
b. / helium / d. / fluorine

____48.Which of the following elements has the smallest ionic radius?

a. / Li / c. / O
b. / K / d. / S

____49.What is the energy required to remove an electron from an atom in the gaseous state called?

a. / nuclear energy / c. / shielding energy
b. / ionization energy / d. / electronegative energy

____50.For Group 2A metals, which electron is the most difficult to remove?

a. / the first
b. / the second
c. / the third
d. / All the electrons are equally difficult to remove.

____51.Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?

a. / increase in atomic size
b. / increase in size of the nucleus
c. / increase in number of protons
d. / fewer electrons in the highest occupied energy level

____52.Which of the following elements has the smallest first ionization energy?

a. / sodium / c. / potassium
b. / calcium / d. / magnesium

____53.Which of the following elements has the lowest electronegativity?

a. / lithium / c. / bromine
b. / carbon / d. / fluorine

____54.Which statement is true about electronegativity?

a. / Electronegativity is the ability of an anion to attract another anion.
b. / Electronegativity generally increases as you move from top to bottom within a group.
c. / Electronegativity generally is higher for metals than for nonmetals.
d. / Electronegativity generally increases from left to right across a period.

____55.Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.

a. / lower / c. / the same
b. / higher / d. / unpredictable

____56.Which of the following decreases with increasing atomic number in Group 2A?

a. / shielding effect / c. / ionization energy
b. / ionic size / d. / number of electrons

____57.Which of the following statements correctly compares the relative size of an ion to its neutral atom?

a. / The radius of an anion is greater than the radius of its neutral atom.
b. / The radius of an anion is identical to the radius of its neutral atom.
c. / The radius of a cation is greater than the radius of its neutral atom.
d. / The radius of a cation is identical to the radius of its neutral atom.

____58.Which of the following factors contributes to the increase in ionization energy from left to right across a period?

a. / an increase in the shielding effect
b. / an increase in the size of the nucleus
c. / an increase in the number of protons
d. / fewer electrons in the highest occupied energy level

____59.As you move from left to right across the second period of the periodic table ____.

a. / ionization energy increases / c. / electronegativity decreases
b. / atomic radii increase / d. / atomic mass decreases

____60.Of the following elements, which one has the smallest first ionization energy?

a. / boron / c. / aluminum
b. / carbon / d. / silicon

Essay

61.Describe the trends in the atomic size of elements within groups and across periods in the periodic table. Provide examples.

62.Explain how ions form. Provide examples.

63.Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide examples.

64.Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the atoms from which they are formed. Explain why this is so.

65.Describe the trends in electronegativity within groups and across periods in the periodic table. Provide examples.