Chemistry (B) Study Guide
Second Trimester Exam March 14
The exam will ask 120 questions from chapters 6 thru 9. Questions will be based on this study guide.
Matching
Match each item with the correct statement below.
a. / electronegativity / f. / periodic lawb. / 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
Match each item with the correct statement below.
a. / halide ion / e. / valence electronb. / octet rule / f. / coordination number
c. / ionic bond / g. / metallic bond
d. / electron dot structure
____11.an electron in the highest occupied energy level of an atom
____12.Atoms react so as to acquire the stable electron structure of a noble gas.
____13.a depiction of valence electrons around the symbol of an element
____14.an anion of chlorine or other halogen
____15.the force of attraction binding oppositely charged ions together
____16.the attraction of valence electrons for metal ions
____17.the number of ions of opposite charge surrounding each ion in a crystal
Match each item with the correct statement below.
a. / coordinate covalent bond / d. / single covalent bondb. / double covalent bond / e. / polar bond
c. / structural formula / f. / hydrogen bond
____18.a depiction of the arrangement of atoms in molecules and polyatomic ions
____19.a covalent bond in which only one pair of electrons is shared
____20.a covalent bond in which two pairs of electrons are shared
____21.a covalent bond in which the shared electron pair comes from only one of the atoms
____22.a covalent bond between two atoms of significantly different electronegativities
____23.a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA
Match each item with the correct statement below.
a. / network solid / e. / tetrahedral angleb. / bonding orbital / f. / VSEPR theory
c. / dipole interaction / g. / sigma bond
d. / bond dissociation energy
____24.energy needed to break a single bond between two covalently bonded atoms
____25.symmetrical bond along the axis between the two nuclei
____26.molecular orbital that can be occupied by two electrons of a covalent bond
____27.109.5
____28.shapes adjust so valence-electron pairs are as far apart as possible
____29.attraction between polar molecules
____30.crystal in which all the atoms are covalently bonded to each other
Match each item with the correct statement below.
a. / monatomic ion / f. / cationb. / acid / g. / binary compound
c. / base / h. / anion
d. / law of definite proportions / i. / polyatomic ion
e. / law of multiple proportions
____31.consists of a single atom with a positive or negative charge
____32.atom or group of atoms having a negative charge
____33.atom or group of atoms having a positive charge
____34.tightly-bound group of atoms that behaves as a unit and carries a net charge
____35.compound composed of two different elements
____36.produces a hydrogen ion when dissolved in water
____37.produces a hydroxide ion when dissolved in water
____38.In any chemical compound, the masses of elements are always in the same proportion by mass.
____39.when two elements form more than one compound, the masses of one element that combine with the same mass of the other element are in the ratio of small, whole numbers
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____40.What is another name for the representative elements?
a. / Group A elements / c. / Group C elementsb. / Group B elements / d. / transition elements
____41.What is another name for the transition metals?
a. / noble gases / c. / Group B elementsb. / Group A elements / d. / Group C elements
____42.Which of the following elements is in the same period as phosphorus?
a. / carbon / c. / nitrogenb. / magnesium / d. / oxygen
____43.Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
a. / Henry Moseley / c. / John Daltonb. / Antoine Lavoisier / d. / Dmitri Mendeleev
____44.Which of the following categories includes the majority of the elements?
a. / metalloids / c. / metalsb. / liquids / d. / nonmetals
____45.Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. / Pt / c. / Lib. / V / d. / Kr
____46.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 electronsb. / Zn, 30 protons, 60 electrons / d. / F, 19 protons, 19 electrons
____47.The atomic number of an element is the total number of which particles in the nucleus?
a. / neutrons / c. / electronsb. / protons / d. / protons and electrons
____48.What element has the electron configuration 1s2s2p3s3p?
a. / nitrogen / c. / siliconb. / selenium / d. / silver
____49.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.
____50.Which of the following electron configurations is most likely to result in an element that is relatively inactive?
a. / a half-filled energy sublevelb. / a filled energy sublevel
c. / one empty and one filled energy sublevel
d. / a filled highest occupied principal energy level
____51.Which subatomic particle plays the greatest part in determining the properties of an element?
a. / proton / c. / neutronb. / electron / d. / none of the above
____52.Which of the following elements is a transition metal?
a. / cesium / c. / telluriumb. / copper / d. / tin
____53.Which of the following groupings contains only representative elements?
a. / Cu, Co, Cd / c. / Al, Mg, Lib. / Ni, Fe, Zn / d. / Hg, Cr, Ag
____54.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.
____55.What are the Group 1A and Group 7A elements examples of?
a. / representative elements / c. / noble gasesb. / transition elements / d. / nonmetallic elements
____56.Of the elements Fe, Hg, U, and Te, which is a representative element?
a. / Fe / c. / Ub. / Hg / d. / Te
____57.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.
____58.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.
____59.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.
____60.Atomic size generally ____.
a. / increases as you move from left to right across a periodb. / 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
____61.What element in the second period has the largest atomic radius?
a. / carbon / c. / potassiumb. / lithium / d. / neon
____62.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 levelb. / an increase in size of the nucleus
c. / an increase in number of protons
d. / fewer electrons in the highest occupied energy level
____63.Which of the following elements has the smallest atomic radius?
a. / sulfur / c. / seleniumb. / chlorine / d. / bromine
____64.What is the charge of a cation?
a. / a positive chargeb. / no charge
c. / a negative charge
d. / The charge depends on the size of the nucleus.
____65.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.
____66.The metals in Groups 1A, 2A, and 3A ____.
a. / gain electrons when they form ions / c. / all have ions with a 1 chargeb. / all form ions with a negative charge / d. / lose electrons when they form ions
____67.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.
____68.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.
____69.In which of the following sets are the charges given correctly for all the ions?
a. / Na, Mg, Al / c. / Rb, Ba, Pb. / K, Sr, O / d. / N, O, F
____70.In which of the following groups of ions are the charges all shown correctly?
a. / Li, O, S / c. / K, F, Mgb. / Ca, Al, Br / d. / Na, I, Rb
____71.What is the element with the lowest electronegativity value?
a. / cesium / c. / calciumb. / helium / d. / fluorine
____72.What is the element with the highest electronegativity value?
a. / cesium / c. / calciumb. / helium / d. / fluorine
____73.Which of the following elements has the smallest ionic radius?
a. / Li / c. / Ob. / K / d. / S
____74.What is the energy required to remove an electron from an atom in the gaseous state called?
a. / nuclear energy / c. / shielding energyb. / ionization energy / d. / electronegative energy
____75.For Group 2A metals, which electron is the most difficult to remove?
a. / the firstb. / the second
c. / the third
d. / All the electrons are equally difficult to remove.
____76.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 sizeb. / increase in size of the nucleus
c. / increase in number of protons
d. / fewer electrons in the highest occupied energy level
____77.Which of the following elements has the smallest first ionization energy?
a. / sodium / c. / potassiumb. / calcium / d. / magnesium
____78.Which of the following elements has the lowest electronegativity?
a. / lithium / c. / bromineb. / carbon / d. / fluorine
____79.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.
____80.Which of the following decreases with increasing atomic number in Group 2A?
a. / shielding effect / c. / ionization energyb. / ionic size / d. / number of electrons
____81.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.
____82.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 effectb. / 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
____83.As you move from left to right across the second period of the periodic table ____.
a. / ionization energy increases / c. / electronegativity decreasesb. / atomic radii increase / d. / atomic mass decreases
____84.Of the following elements, which one has the smallest first ionization energy?
a. / boron / c. / aluminumb. / carbon / d. / silicon
____85.How many valence electrons are in an atom of phosphorus?
a. / 2 / c. / 4b. / 3 / d. / 5
____86.How many valence electrons are in an atom of magnesium?
a. / 2 / c. / 4b. / 3 / d. / 5
____87.How many valence electrons does a helium atom have?
a. / 2 / c. / 4b. / 3 / d. / 5
____88.How many valence electrons are in a silicon atom?
a. / 2 / c. / 6b. / 4 / d. / 8
____89.What is the name given to the electrons in the highest occupied energy level of an atom?
a. / orbital electrons / c. / anionsb. / valence electrons / d. / cations
____90.How does calcium obey the octet rule when reacting to form compounds?
a. / It gains electrons.b. / It gives up electrons.
c. / It does not change its number of electrons.
d. / Calcium does not obey the octet rule.
____91.What is the maximum charge an ion is likely to have?
a. / 2 / c. / 4b. / 3 / d. / 5
____92.What is the charge on the strontium ion?
a. / 2– / c. / 1b. / 1– / d. / 2
____93.How many electrons does silver have to give up in order to achieve a pseudo-noble-gas electron configuration?
a. / 1 / c. / 3b. / 2 / d. / 4
____94.How many electrons does barium have to give up to achieve a noble-gas electron configuration?
a. / 1 / c. / 3b. / 2 / d. / 4
____95.What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a. / K / c. / Kb. / K / d. / K
____96.Which of the following ions has a pseudo-noble-gas electron configuration?
a. / Fe / c. / Cub. / Mn / d. / Ni
____97.Which of the following elements does NOT form an ion with a charge of 1?
a. / fluorine / c. / potassiumb. / hydrogen / d. / sodium
____98.What is the formula of the ion formed when tin achieves a stable electron configuration?
a. / Sn / c. / Snb. / Sn / d. / Sn
____99.What is the formula of the ion formed when cadmium achieves a pseudo-noble-gas electron configuration?
a. / Cd / c. / Cdb. / Cd / d. / Cd
____100.How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
a. / 1 / c. / 3b. / 2 / d. / 4
____101.What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?
a. / P / c. / Pb. / P / d. / P
____102.How does oxygen obey the octet rule when reacting to form compounds?
a. / It gains electrons.b. / It gives up electrons.
c. / It does not change its number of electrons.
d. / Oxygen does not obey the octet rule.
____103.What is the charge on the cation in the ionic compound sodium sulfide?
a. / 0 / c. / 2b. / 1 / d. / 3
____104.Which of the following occurs in an ionic bond?
a. / Oppositely charged ions attract.b. / Two atoms share two electrons.
c. / Two atoms share more than two electrons.
d. / Like-charged ions attract.
____105.What is the net charge of the ionic compound calcium fluoride?
a. / 2– / c. / 0b. / 1– / d. / 1
____106.Which of the following is true about an ionic compound?
a. / It is a salt. / c. / It is composed of anions and cations.b. / It is held together by ionic bonds. / d. / all of the above
____107.How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?
a. / 0 / c. / 2b. / 1 / d. / 3
____108.How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide?
a. / 0 / c. / 2b. / 1 / d. / 3
____109.What is the formula unit of sodium nitride?
a. / NaN / c. / NaNb. / NaN / d. / NaN
____110.What is the formula unit of aluminum oxide?
a. / AlO / c. / AlOb. / AlO / d. / AlO
____111.What is the name of the ionic compound formed from lithium and bromine?
a. / lithium bromine / c. / lithium bromiumb. / lithium bromide / d. / lithium bromate
____112.What is the formula for sodium sulfate?
a. / NaSO / c. / Na(SO)b. / NaSO / d. / Na(SO)
____113.What is the formula for potassium sulfide?
a. / KS / c. / KSb. / KS / d. / KS
____114.Which of the following compounds has the formula KNO?
a. / potassium nitrate / c. / potassium nitriteb. / potassium nitride / d. / potassium nitrogen oxide
____115.Which of the following pairs of elements is most likely to form an ionic compound?
a. / magnesium and fluorine / c. / oxygen and chlorineb. / nitrogen and sulfur / d. / sodium and aluminum
____116.Ionic compounds are normally in which physical state at room temperature?
a. / solid / c. / gasb. / liquid / d. / plasma
____117.What does the term coordination number in ionic crystals refer to?
a. / the total number of valence electrons in an atomb. / the number of oppositely charged ions surrounding a particular ion
c. / the number of atoms in a particular formula unit
d. / the number of like-charged ions surrounding a particular ion
____118.Under what conditions can potassium bromide conduct electricity?
a. / only when meltedb. / only when dissolved
c. / only when it is in crystal form
d. / only when melted or dissolved in water
____119.Which of the following is NOT a characteristic of most ionic compounds?
a. / They are solids.b. / They have low melting points.
c. / When melted, they conduct an electric current.
d. / They are composed of metallic and nonmetallic elements.
____120.Which of the following particles are free to drift in metals?
a. / protons / c. / neutronsb. / electrons / d. / cations
____121.What is the basis of a metallic bond?
a. / the attraction of metal ions to mobile electronsb. / the attraction between neutral metal atoms
c. / the neutralization of protons by electrons
d. / the attraction of oppositely charged ions
____122.What characteristic of metals makes them good electrical conductors?
a. / They have mobile valence electrons.b. / They have mobile protons.
c. / They have mobile cations.
d. / Their crystal structures can be rearranged easily.
____123.Which metallic crystal structure has a coordination number of 8?
a. / body-centered cubic / c. / hexagonal close-packingb. / face-centered cubic / d. / tetragonal
____124.Which is a typical characteristic of an ionic compound?
a. / Electron pairs are shared among atoms.b. / The ionic compound has a low solubility in water.
c. / The ionic compound is described as a molecule.
d. / The ionic compound has a high melting point.
____125.What is shown by the structural formula of a molecule or polyatomic ion?
a. / the arrangement of bonded atoms / c. / the number of metallic bondsb. / the number of ionic bonds / d. / the shapes of molecular orbitals
____126.Which of these elements does not exist as a diatomic molecule?
a. / Ne / c. / Hb. / F / d. / I
____127.How do atoms achieve noble-gas electron configurations in single covalent bonds?
a. / One atom completely loses two electrons to the other atom in the bond.b. / Two atoms share two pairs of electrons.
c. / Two atoms share two electrons.
d. / Two atoms share one electron.
____128.Why do atoms share electrons in covalent bonds?
a. / to become ions and attract each otherb. / to attain a noble-gas electron configuration
c. / to become more polar
d. / to increase their atomic numbers
____129.Which of the following elements can form diatomic molecules held together by triple covalent bonds?