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Unit 3 Practice Questions
Ionic Bonding Questions 1-3 refer to the following: X+ X+2 X+3 XO3-2 XO4-2 A type of ion found in sodium acetate A type of ion found in aluminum oxide A type of ion found in potassium phosphate
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Questions 1-2 refer to the following: 1 7 9 10 14
The atomic number of an atom with an electron dot arrangement similar to iodine The number of atoms represented in the formula Al(OH)3 Basic measurements A E C B
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Questions 1-4 refer to the following: Na+ Al F Ti Br--
Has 7 valence electrons Has the electron configuration 1s22s22p63s23p1 Has the same electron configuration as a neon atom Has valence electrons in d orbitals Basic measurements A E C B
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Questions 1-5 refer to the following: Ca+ and K H+ and He Cl- and F
O- and S+ Na+ and O-- Difference of 6 electrons Same number of electrons Difference of 9 electrons Difference of 2 electrons Difference of 1 electron Basic measurements A E C B
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Molten sodium chloride is a good electrical conductor II
Sodium chloride in the molten state allows ions to move freely BECAUSE Sodium chloride is an example of ionic bonding Sodium and chlorine have the same electronegativity BECAUSE Density T,F F,T
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An ionic solid is a good conductor of electricity II
An ionic solid is composed of positive and negative ions joined together in a lattice structure held together by electrostatic forces BECAUSE When a chlorine atom gains an electron, it becomes a positively charged ion A neutral atom has equal numbers of protons and electrons BECAUSE Density T,F F,T
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Crystals of sodium chloride go into solution in water as ions II
The sodium ion has a 1+ charge and the chloride ion has a 1- charge and they are hydrated by the water molecules BECAUSE For an element with an atomic number of 17, the most probable oxidation number (charge) is +1 The outer energy level of the halogen family has a tendency to add one electron to itself BECAUSE Density T,F F,T
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The ionic bond is the strongest bond II
Ionic bonds have electrostatic attraction due to the loss and gain of electrons BECAUSE Atom A with 7 valence electrons forms AB2 with atom B with two valence electrons B donates its electrons to fill the outer shell of A BECAUSE Density T,F F,T
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MgO has a high melting point II
Highly charged ions result in strong ionic forces and high lattice energies BECAUSE A solution of NaCl will conduct electricity NaCl will not form ions in solution BECAUSE Density T,F F,T
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The correct formula for calcium hydrogen sulfate is CaH2SO4 CaHSO4
Density E
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Which sample below has its atoms arranged in a regular, geometric pattern?
NaC2H3O2 (s) H2O (l) Ar (g) NaCl (aq) CH4 (g) Density E
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How many electrons does a 37Cl ion with a charge of -1 contain?
16 17 18 37 38 Density E
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Which element is most likely represented by X in the oxygen-containing ion, XO4-3?
Cl Density E
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Which of the following is NOT true of the element sodium?
It takes the oxidation state (charge) +1 It reacts with water to form a basic solution It forms metallic bonds in its solid uncombined form It is found in nature as a diatomic gas It reacts with a halogen to form an ionic salt Density E
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How many atoms are present in the formula KAl(SO4)2?
7 9 11 12 13 Density E
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Which sample has atoms that are arranged in a regular geometric pattern?
KCl (l) NaC2H3O2 (s) Fe (l) NaCl (aq) HCl (aq) Density E
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Hydrated molecules only Dehydrated ions and molecules
When an ionic compound is dissolved in water, the ions in solution can best be described as Hydrated molecules only Dehydrated ions and molecules Both hydrated molecules and hydrated ions Neither hydrated ions nor hydrated molecules Hydrated ions only Density E
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What is the chemical formula for iron(III) sulfate? Fe2SO4 Fe3SO4
Density E
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The name of the compound MgBr2 is Manganese bromite Manganese bromide
Magnesium bromite Magnesium bromide Magnesium dibromide Density E
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The anion S2- is called Sulfide Sulfite Sulphorous Sulfuron Sulfate
Density E
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Element X forms the compounds XCl3 and X2O3
Element X forms the compounds XCl3 and X2O3. Element X would most likely belong to the group called Alkali metals Alkaline earth metals Group 13 Halogens Noble gases Density E
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A nonmetal (X) reacts with a metal (M) to give the formula M2X
A nonmetal (X) reacts with a metal (M) to give the formula M2X. Which pairing below is most like elements represented by M and X? Ca and N Li and S Si and O Rb and F Mg and Cl Density E
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In the Lewis dot structure X: , what is the predictable oxidation number (charge)?
+1 -1 +2 -2 +3 Density E
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Which of the following compounds would be expected to have the greatest lattice binding energy?
LiNO3 LiF KI NH4Br CsNO3 Density E
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They contain the same number of protons
Which of the following is true regarding an Ne atom with a mass number of 20 and an O2- ion with a mass number of 16? They contain the same number of protons They contain the same number of neutrons They contain the same number of protons plus neutrons They are isoelectronic They are isomers Density E
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Which bonds are ionic? I. HCl II. SCl III. CsF I only III only
I and II only II and III only I, II and III Substance B
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Questions 1-3 refer to the following: CH4 CO2 NH3 N2 O2
II. Covalent Bonding Questions 1-3 refer to the following: CH4 CO2 NH3 N2 O2 Forms hydrogen bonds Is polar Has a triple bond Safety A E D
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Ammonia (NH3) has a trigonal pyramidal molecular structure
A pi bond is formed between the lobes of adjacent p orbitals in the same plane of two atoms that contain only one electron each II Each of the two lobes of a single p orbital can hold two electrons of opposite spin BECAUSE Ammonia (NH3) has a trigonal pyramidal molecular structure BECAUSE Ammonia has a tetrahedral electron pair geometry with three atoms bonded to the central atom Density T,F F,T
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SO3 is very unstable and resonates between these possible structures
Maximum repulsion between two electron pairs in a molecular compound will result in a linear structure II The VSEPR model says that like charges will orient themselves so as to diminish the repulsion between them BECAUSE The structure of SO3 is shown by using more than one structural formula BECAUSE SO3 is very unstable and resonates between these possible structures Density T,F F,T
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C2H2 is a linear compound with a triple bond between the carbons
The hybrid orbital form of carbon in acetylene (C2H2) is believed to be the sp form II C2H2 is a linear compound with a triple bond between the carbons BECAUSE The weakest of the bonds between molecules are coordinate covalent bonds Coordinate covalent bonds represent the weak attractive force of the electrons of one molecule for the positively charged nucleus of another BECAUSE Density T,F F,T
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Water is a polar substance II
The sharing of the bonding electrons in water is equal BECAUSE Water is a good solvent for ionic and/or polar covalent substances Water shows hydrogen bonding between oxygen atoms BECAUSE Density T,F F,T
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The atomic radius of H is smaller than the atomic radius of N
The N-N bond distance in N2 is shorter than the N-N bond distance in N2H4 II The atomic radius of H is smaller than the atomic radius of N BECAUSE Elemental iodine has a higher boiling point than elemental bromine Iodine forms stronger covalent bonds than bromine BECAUSE Density T,F F,T
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The boiling point of H2O is higher than the boiling point of H2S II
H2S has a greater molecular mass than H2O BECAUSE Bromine has a higher boiling point than chlorine Bromine has higher dispersion forces than chlorine BECAUSE Density T,F F,T
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Some covalent bonds are polar in nature II
Atoms of different electronegativities are unequal in the degree to which they attract electrons BECAUSE A nonpolar molecule can have polar bonds Polar bonds can be symmetrically arranged in a molecule so that there are no net poles BECAUSE Density T,F F,T
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The bond in an O2 molecule is nonpolar II
The oxygen atoms in an O2 molecule share the bonding electrons equally BECAUSE BF3 has a tetrahedral geometry The central B atom does not have a complete stable octet BECAUSE Density T,F F,T
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Extra energy is necessary to break the hydrogen bonds
Substances with hydrogen bonding tend to have unusually low boiling points II Extra energy is necessary to break the hydrogen bonds BECAUSE CCl4 is a nonpolar compound The dipole moments are canceled out BECAUSE Density T,F F,T
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A tetrahedral molecule, XY4, would be formed if X were using the orbital hybridization
p2 s2 sp sp2 sp3 Conversion D
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Which of the elements below is most likely to form compounds in which it has an incomplete octet?
Conversion D
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Which substance has a polar covalent bond between its atoms?
K3N Ca3N2 NaCl F2 NH3 Conversion D
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Which molecule is a polar molecule? N2 H2O CH4 CO2 KCl
Conversion D
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In which of the following compounds are hydrogen bonds between molecules the strongest?
HF HCl HBr HI HAt Conversion D
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The compound PF5 is called Monophorofluoride Phosphorus pentafluoride
Pentaphosphoro fluoride Phosphorus tetrafluoride Potassium pentafluoride Conversion D
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How many sigma and pi bonds are found in the following molecule?
H—C C—CH2—CH=CH2 6 sigma, 2 pi 2 sigma, 6 pi 10 sigma, 3 pi 5 sigma, 3 pi 11 sigma, 2 pi Conversion D
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Which of the following statements is false? H2 has just one sigma bond
HCl has just one sigma bond H—C C—H has four pi and three sigma bonds CH2=CH2 has five sigma bonds and one pi bond H2O has two sigma bonds and two lone pairs Conversion D
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How many pi bonds are there in a molecule of N C—CH2—CH2—NH—CH=CH2 6 4
12 10 3 Conversion D
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Which of the following species has a molecular shape most similar to that of ammonia, NH3?
BH3 H2O H3O+ CH4 NH4+ Conversion D
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Which compound below has a bent molecular geometry?
H2SO4 CH4 CO2 H2S C2H2 Conversion D
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Which compound of oxygen is most likely to contain an O-O bond?
SO2 H2O2 TiO2 Conversion D
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How many single bonds are in a molecule of carbon dioxide, CO2?
None One Two Three Four Conversion D
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All of the following have covalent bonds EXCEPT HCl CCl4 H2O CsF CO2
Conversion D
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Which of the following molecules is polar? BH3 NF3 C2H6 SF6 CCl4
Conversion D
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The shape of a PCl3 molecule can be described as Bent
Trigonal pyramidal Linear Trigonal planar Tetrahedral Conversion D
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Which of the following is a nonpolar molecule? CO2 H2O NH3 NO HI
Conversion D
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The structure of SiO2 can best be described as Linear Bent Trigonal
Tetrahedral Square Conversion D
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Which of the following molecules has a trigonal pyramidal geometry?
BH3 H2O CH4 NH3 AlCl3 Conversion D
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Which of these resembles the molecular structure of the water molecule?
H—H—O, linear H—O—H, bent, 30o angle H—O—H, bent, 90o angle H—O—H, bent, 105o angle H—O—H, linear Conversion D
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The shape of a PCl3 molecule is described as Bent Trigonal planar
Linear Trigonal pyramidal tetrahedral Conversion D
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The bond that includes an upper and a lower sharing of electron orbitals is called
A pi bond A sigma bond A hydrogen bond A covalent bond An ionic bond Conversion D
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What is the structure associated with the BF3 molecule?
Linear Trigonal planar Tetrahedron Trigonal pyramidal Bent Conversion D
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The new orbitals are one s orbital and three p orbitals
Which of these statements is the best explanation for the sp3 hybridization of carbon’s electrons? The new orbitals are one s orbital and three p orbitals The s electron is promoted to the p orbitals The s orbital is deformed into a p orbital Four new and equivalent orbitals are formed The s orbital electron loses energy to fall back into a partially filled p orbital Conversion D
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Coordinate covalent bonding
The intermolecular force that is most significant in explaining the variation of the boiling point of water from the boiling points of similarly structured molecules is Hydrogen bonding Van der Waals forces Covalent bonding Ionic bonding Coordinate covalent bonding Conversion D
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Which of the following properties can be attributed to water?
I. It has a permanent dipole moment attributed to its molecular structure II. It is a very good conductor of electricity III. It has polar covalent bonds with hydrogen on opposite sides of the oxygen atom, so that the molecule is linear I only III only I and II only II and III only I, II and III Substance B
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III. All Types of Bonding Questions 1-3 refer to the following:
Ionic substance Metallic substance Polar covalent molecule Nonpolar covalent molecule Aromatic organic molecule Carbon tetrachloride Cesium chloride Hydrogen chloride Basic measurements (similar to slide 1) A B C E
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Questions 1-4 refer to the following: Ionic Covalent Polar covalent
Metallic Hydrogen bonding When the electronegativity difference between 2 atoms is 2 If two atoms are bonded in such a way that both members of the pair equally share one electron with the other Which of the 5 choices is the weakest bond? If an electron is lost by one atom and completely captured by another Basic measurements (similar to slide 1) A B C E
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Questions 1-3 refer to the following: Water Hydrogen bromide Iron
Argon Sodium chloride Hydrogen bonding Highly polar Dispersion forces Basic measurements (similar to slide 1) A B C E
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Questions 1-3 refer to the following: Ionic Covalent Polar covalent
Metallic Hydrogen bonding Bonding that explains water’s high boiling point If the sharing of an electron pair is unequal and the atoms have an electronegativity difference of 1.4 to 1.6 If one or more valence electrons become detached from the atoms and migrate in a “sea” of free electrons among the positive metal ions Basic measurements (similar to slide 1) A B C E
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Questions 1-3 refer to the following: Hydrogen gas, H2
Carbon monoxide, CO Potassium, K Aluminum oxide, Al2O3 Bromine, Br2 Substance held together by metallic bonds Substance held together by ionic bonds Consists of polar molecules Basic measurements (similar to slide 1) A B C E
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Questions 1-4 refer to the following: Hydrogen bond Ionic bond
Polar covalent bond Nonpolar covalent bond Metallic bond The type of bond between atoms of potassium and chloride The type of bond between the atoms in a nitrogen molecule The type of bond between the atoms in CO2 (electronegativity difference = 1) The type of bond between the atoms of calcium in a crystal of calcium Basic measurements (similar to slide 1) A B C E
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Questions 1-4 refer to the following: Ionic substance
Polar covalent substance Nonpolar covalent substance Amorphous substance Metallic network KCl (s) HCl (g) CH4 (g) Li (s) Basic measurements (similar to slide 1) A B C E
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Questions 1-4 refer to the following: Hydrogen bonding Ionic bonding
Metallic bonding Nonpolar covalent bonding Polar covalent bonding Holds a sample of barium iodide, BaI2, together Allows solids to conduct electricity Attracts atoms of hydrogen to each other in an H2 molecule Responsible for relatively low vapor pressure of water Basic measurements (similar to slide 1) A B C E
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Questions 1-5 refer to the following: Hydrogen bonding Ionic bonding
Network bonding London dispersion force Metallic bonding Chiefly responsible for the relatively high boiling point of water Is present in liquid oxygen Is primarily responsible for the hardness of diamond Allows copper to conduct electricity Is present in solid KCl Basic measurements (similar to slide 1) A B C E
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Ionic bonds are always stronger than covalent bonds
Most atoms are less stable in the bonded state than in the unbonded state II Both ionic and covalent bonds fail to provide the participating atoms with a stable electron configuration BECAUSE Ionic bonds are always stronger than covalent bonds BECAUSE They break only when bombarded with electrons Density T,F F,T
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I The most important factor in determining the chemical properties of an element is the number of electrons in the outermost shell II The number of electrons in the outer shell determines the bonding characteristics of the element BECAUSE Density T,F F,T Helium will have fewer dispersion forces between its atoms than the other noble gases As the mass of nonpolar atoms and molecules increases, dispersion forces increase BECAUSE
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Which of the following are the WEAKEST attractive force?
Dipole-dipole forces Coordinate covalent bonding Covalent bonding Polar covalent bonding Ionic bonding Conversion D
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A coordinate covalent bond A pi bond between p orbitals
The complete loss of an electron of one atom to another atom with the consequent formation of electrostatic charges is referred to as A covalent bond A polar covalent bond An ionic bond A coordinate covalent bond A pi bond between p orbitals Conversion D
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Which of the following compounds would be predicted to have the highest melting point?
CS2 HI H2S H2O MgO Conversion D
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Which compound is not paired with its correct name?
FeCl2 / iron(II) chloride K2O / potassium oxide NO2 / nitrogen dioxide PCl3 / potassium trichloride NH4Cl / ammonium chloride Conversion D
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Which of the following statements about bonding is correct?
Van der Waals forces exist between polar molecules Dipoles are the result of the equal sharing of electrons Cu(s) is a network solid Hydrogen bonds exist between the molecules of HCl NaCl (aq) has attraction between the molecules and the ions Conversion D
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Which kinds of bonding can be found in a sample of H2O (l)?
Hydrogen bonds only Nonpolar covalent bonds only Ionic and nonpolar hydrogen bonds Both polar covalent and hydrogen bonds Metallic and ionic bonds Conversion D
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Which compound contains no ionic character? NH4Cl CaO K2O Li2O CO
Conversion D
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Van der Waals/ dispersion forces Ionic bonds Covalent bonds
The forces of attraction that exist between nonpolar molecules are called Van der Waals/ dispersion forces Ionic bonds Covalent bonds Electrovalent bonds Metallic bonds Conversion D
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When a salt dissolves in water, the water molecules are attracted by ions in solution. This attraction is called Atom-atom Molecule-molecule Molecule-ion Ion-ion Atom-ion Conversion D
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Which element is expected to have a “sea” of electrons?
Hydrogen Nitrogen Cobalt Chlorine Oceanium Conversion D
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In which of the following liquids are the Van der Waals forces of attraction between the molecules weakest? Xe Kr Ar Ne He Conversion D
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Which molecule has both nonpolar intramolecular and nonpolar intermolecular bonds?
CCl4 CO HF HCl F2 Conversion D
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If two atoms that differ in electronegativity combine by chemical reaction and share electrons, the bond that joins them will be Metallic Ionic A hydrogen bond Nonpolar covalent Polar covalent Conversion D
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The number of protons in the nucleus
The reactivity and chemical behavior of an atom is governed by many factors. The most important factor is The number of protons in the nucleus The number of neutrons in the nucleus The number of protons and neutrons in the nucleus The ratio of protons and neutrons in the nucleus The number of electrons in the valence shell Conversion D
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