AP Chemistry Brown Chapter 8, Bonding
How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?
4
How many elements in the periodic table are represented by a Lewis symbol with a single dot?
7
There are ______ covalent bonds in the Lewis Structure of CH3CHCl2.
7
The halogens, alkali metals, and alkaline earth metals have ________ valence electrons, respectively.
7, 1, 2
In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________.
+1
The formal charge on nitrogen in NO3- is ________, where the Lewis structure of the ion is: [compound]^-1
+1
The oxidation number of iron in Fe2O3 is ________.
+3
The oxidation number of phosphorus in PF5 is ________.
+5
Draw the Lewis structure of ICl2 +.
-- o o o o o o -- | o Cl _____ I _____ Cl o | | o o | -- o o o o o o --
A triple bond consists of ________ pairs of electrons shared between two atoms.
3
How many equivalent resonance forms can be drawn for CO32-? (Carbon is the central atom.)
3
How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom?
3
How many single covalent bonds must a nitrogen atom form to have a complete octet in its valence shell?
3
What is the bond order of N2?
3
The ion ICl4- has ________ valence electrons.
36
Consider ion 5. How many attractive electrostatic interactions are shown for it?
4
Consider ion 5. How many repulsive interactions are shown for it?
4
There are ________ paired and ________ unpaired electrons in the Lewis symbol for a oxygen atom.
4, 2
How many dots should be shown in the Lewis symbol for phosphorus?
5
The principal quantum number of the electrons that are lost when yttrium forms a cation is ________.
5
The N−Nbond length in N2O is 1.12 Å, slightly longer than a typical N≡N bond; and the N−ON−O bond length is 1.19 Å slightly shorter than a typical bond (see Table 8.5 in the textbook). Based on these data, which resonance structure best represents N2O? a. 2e^- - N≡N - O 6e^- b. 6e^- N - N≡O 2e^- c. 2e^- =N=O 2e^-
All
Describe the electron transfers that occur in the formation of calcium fluoride from elemental calcium and elemental fluorine.
Each Ca atom transfers one electron to each of two fluorine atoms.
Consider the covalent bond each of the following elements forms with hydrogen: chlorine, phosphorus, sulfur, and silicon. Which will form the most polar bond with hydrogen? S, Cl, Si, P
Cl
The ________ ion has a noble gas electron configuration.
Cl-
A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
ClF3
A substance XY, formed from two different elements, boils at -33 ∘C. Is XY likely to be a covalent or an ionic substance?
Covalent
Phosphorus pentchloride (PCl5PCl5) is used as a chlorinating reagent in chlorination of organic compounds. What type of bonding occurs between the atoms of a PCl5PCl5 molecule?
Covalent
State whether the bonding in each compound is likely to be covalent or not: iron, water, oxygen, sodium chloride, argon,
Covalent: water, oxygen Not Covalent: iron, sodium chloride, argon
The ________ ion is represented by the electron configuration [Ar]3d2.
Cr4+
In which of the molecules below is the carbon-carbon distance the shortest?
H-C≡≡C-H
Which of these molecules has the same number of shared and unshared electron pairs?
H2S
If molecule A has a bond enthalpy of 418 kJ/mol and molecule B has a bond enthalpy of 941 kJ/mol, what can be said of molecule A compared to molecule B?
It requires less energy to break the bonds in molecule A than it does in molecule B.
Which of these elements is unlikely to form covalent bonds?S, H, K, Ar, Si
K and Ar
Which of the following shows the correct order of increasing lattice energy for the given compounds?
K2O < Na2O < Li2O
The chloride of which of the following metals should have the greatest lattice energy?
Lithium
The Lewis structure of HCN (H bonded to C) shows that ________ has ________ nonbonding electron pair(s).
N, 1
The lattice energies of NaCl and KF are given in table below. Based on the lattice energies, would you expect the Na−Cl or the K−F distance to be longer?
Na-Cl
Use the ionic radii given in figure below to estimate the Na−Cl and K−F distances.
Na-Cl: 2.83 K-F: 2.71
Of the following, ________ cannot accommodate more than an octet of electrons.
O
The type of compound that is most likely to contain a covalent bond is ________.
One that is composed of only nonmetals.
If you are told that one of them is Cr2O3 and the other is OsO4, which one do you expect to be the yellow solid?
OsO4
Based on the octet rule, phosphorus most likely forms a ________ ion.
P3-
The central atom in ________ violates the octet rule.
PF5
Rank the atomic radius from largest to smallest: Cl, Pb, Al, F
Pb, Al, Cl, F
The formula of palladium (IV) sulfide is ________.
PdS2
The orbital diagram that follows shows the valence electrons for a 2+ ion of an element. What is the element? [/\\/][/\][/\][/\][/\]
Ru
In which of these molecules or ions is there only one lone pair of electrons on the central sulfur atom?
SF4
Without looking at Table 8.2, predict which one of the following orderings of lattice energy is correct for these ionic compounds.
ScN > MgO > NaCl > CsI
Of the molecules SiCl4 and SiI4, which has bonds that are more polar?
SiCl4
Which of these molecules has a Lewis structure with a central atom having no nonbonding electron pairs? H2S, SiF4, CO2, PF3
SiF4, CO2
A ________ covalent bond between the same two atoms is the longest.
Single
Based on this distance and differences in electronegativity, do you expect the dipole moment of an individual H−CH−C bond to be larger or smaller than that of the H−IH−I bond?
Smaller
Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration?
Sr
Which of the following does not have eight valence electrons?
Sr+
Energy is required to remove two electrons from Ca to form Ca2+, and energy is required to add two electrons to O to form O2− . Yet CaOis stable relative to the free elements. Which statement is the best explanation?
The lattice energy of CaO is large enough to overcome these processes.
If you were to perform the reaction LiCl (s)→Li(s)→Li(g)+ Cl−(g), would energy be absorbed or released?
absorbed
Which two would form the longest single bond? a. P-O b. Te-I c. B-O d. P-I
b. Te-I
If no color key were provided, is there a way for you to guess whether the green spheres represent Na+ or Cl−? If so, what information would you use?
cations have a {smaller} radius... anions have a {large}... we would expect {Na+}... smaller than {Cl-}... represent {Cl-}
Of the possible bonds between carbon atoms (single, double, and triple), ________.
double is stronger than triple
A nonpolar bond will form between two ________ atoms of ________ electronegativity.
identical, equal
In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________.
increase, increase, decrease
Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.
increases, decreases
For a given arrangement of ions, the lattice energy decreases as ionic radius ________ and as ionic charge ________.
increases, decreases
Elements from opposite sides of the periodic table tend to form ________.
ionic compounds
Which combinations of elements would likely yield a compound of empirical formula X2Y3? a. B2O3 and P2O3 b. B2I3 and P2I3 c. B2O3 and P2I3 d. B2I3 and P2O3
its either a or c i forget sorry
Is the sum of the attractive interactions in part (c) larger or smaller than the sum of the repulsive interactions in part (d)?
larger
Resonance structures differ by ________
placement of electrons only
If this pattern of ions was extended indefinitely in two dimensions, would the lattice energy be positive or negative?
positive
A ________ covalent bond between the same two atoms is the longest.
single
Which colored balls must represent sodium ions?
smaller purple
Two possible electron-dot structures are shown for the cyanate ion, NCO−. (Figure 1) What can you conclude about how favorable the structures are? (picture shows structure A, structure B takes four electrons from the oxygen and puts them on the nitrogen)
structure A
Lattice energy is ________.
the energy required to convert a mole of ionic solid into its constituent ions in the gas phase
Using Lewis symbols, diagram the reaction between magnesium and oxygen atoms to give the ionic substance MgOMgO .
the one where the only two electrons from Mg are going to the oxygen with two complete pairs and two lone electrons, to form Mg+2 and [O]^-2
Without drawing a Lewis structure, do you think that CO contains a single, double, or triple bond?
triple
T or F: Electron affinity is a measure of how strongly an atom can attract additional electrons.
true
T or F: Most transition metals do not form ions with a noble gas configuration.
true
The greater the lattice energy, the greater the charges on the participatory ions and the smaller their radii.
true
Of the bonds C-C, C=C, and C≡≡C, the C-C bond is ________.
weakest/longest
Of the bonds C-N, C=N, and C≡≡N, the C-N bond is ________.
weakest/longest
Do you expect a similar reaction between potassium metal and elemental bromine?
yes
Draw the Lewis structure(s) (dont) for the molecule with the chemical formula C2H3NC2H3N, where the NN is connected to only one other atom. How many double bonds are there in the correct Lewis structure?
zero
Calculate the formal charge on the chlorine (Cl) atom.
0
How many lone pairs are on the central atom in BCl3?
0
What is the maximum number of double bonds that a hydrogen atom can form?
0
Calculate the formal charge on each of the oxygen (O) atoms
0, 0, -1
How many electrons should be shown in the Lewis symbol for hydrogen?
1
What is the bond order of F2?
1
What is the maximum number of triple bonds that a carbon atom can form?
1
Which of the following would have to lose three electrons in order to achieve a noble gas electron configuration?
Al
Based on the octet rule, aluminum most likely forms an ________ ion.
Al3+
Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?
B
In the molecule BrI, which atom is the negative pole?
Br
The central atom in ________ does not violate the octet rule.
CF4
Which of the following does not have eight valence electrons?
Ca+
Which of the following atoms could have an expanded octet when it is the central atom in a covalent compound?
Cl
Rank from lest to most electronegative: K, P, Co, F
F, P, Co, K
Which of these molecules has the same number of shared and unshared electron pairs? Br2, CCl2F2, PF3, HCl, H2S
H2S
Of the molecules below, the bond in ________ is the most polar. HI, HBr, HF, H2, HCl
HF
The only noble gas without eight valence electrons is ________.
He
Which of these molecules has the larger dipole moment? ClF or IF
IF
A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
IF3
What type of bonding occurs in magnesium oxide, MgOMgO?
Ionic
Consider the following element combinations. Classify the bonds. Al and N, S and S, S and I, O and Cl, Fe and O, I and I, Cs and Cl, P and Cl,
Ionic: Al and N, Fe and O, Cs and Cl Covalent Non-Polar: O and Cl, P and Cl, S and I Covalent Polar: S and S, I and I
Which of these elements is unlikely to form covalent bonds? S, H, K, Ar, Si
K, Ar
The ________ ion has a noble gas electron configuration.
Li+
Classify the elements: F, Ne, Sn, Te, Ga, Zn
Metal: Zn, Sn, Ga Nonmetal: F, Ne Semi-Metal: Te
What type of bonding occurs in a sample of pure sodium, NaNa? In other words, how is one sodium atom held to another sodium atom?
Metallic
Based on the octet rule, magnesium most likely forms a ________ ion.
Mg2+
Benzene, an aromatic organic compound, is often represented as a hexagon with a circle in it to emphasize which of the following?
That there are two equivalent Lewis structures that can be drawn.
Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2?
That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom
For the group 6A elements, what is the trend in electronegativity with increasing atomic number?
The electronegativity decreases with increasing atomic number.
Which friend is most correct?
The second friend is more correct. Because atomic radius increases going down a family, elements in the third period and beyond have the space and available orbitals to accommodate extra electrons, they are less subject to destabilization from additional electron-electron repulsions.
Without drawing a Lewis structure, do you think that COCO contains a single, double, or triple bond?
Triple
T or F, Electron affinity is a measure of how strongly an atom can attract additional electrons.
True
T or F: As electronegativity difference increases, bond length will decrease.
True
The electron configuration of the phosphide ion (P3-) is _______
[Ne]3s23p6
Which two would form the most polar single bond? a. B-O b. Te-I c. I-O d. P-O
a. B-O
Given the electronegativities below, which covalent single bond is most polar? Element H C N O Electneg: 2.1 2.5 3.0 3.5 a. O-H b. C-H c. O-N
a. O-H
Bond enthalpy is ________.
always positive
All four of the silicon-chlorine single bonds in SiCl4SiCl4 are polar. In which direction should the polarity arrows point?
away from the central silicon atom
The most electronegative atom of the ones listed below is ________. a. TI b. B c. In d. Ga e. Al
b. B
For resonance forms of a molecule or ion, ________.
the observed structure is an average of the resonance forms
T or F: Boron compounds are frequent exceptions to the octet rule because they have too few electrons surrounding the boron.
true
T or F: The octet rule is based on the fact that filling in all s and p valence electrons in a shell gives eight electrons.
true
A double bond consists of ________ pairs of electrons shared between two atoms.
2
How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom? (Sulfur is the central atom.)
2
How many lone pairs are on the central atom of BrF3?
2
How many resonance structures can be drawn for ozone, O3?
2
What is the bond order of O2?
2
What is the maximum number of double bonds that a carbon atom can form?
2
The following three Lewis structures can be drawn for N2O: Which is most important?
2 e- - N triple N - O 6 e-
The formal charge on carbon in the molecule below is ________. ..oo.............oo ..O ==C== O ..oo.............oo
0
The formal charge on sulfur in SO42- is ________, where the Lewis structure of the ion is: [compound] ^ 2-
0
What is the formal charge on the hydrogen atom in HF?
0
In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________.
0, 0
In the Lewis structure of HCO3-, the formal charge on H is ________, and the formal charge on C is ________.
0, 0
What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. Molecule: HOFO
0, 0, 1, -1
In the Lewis symbol for a boron atom, there are ________ paired and ________ unpaired electrons.
0, 3
The Lewis structure of AsH3 shows ________ nonbonding electron pair(s) on As.
1
The Lewis structure of PF3 shows that the central phosphorus atom has ________ nonbonding and ________ bonding electron pair(s)
1, 3
There are ________ valence electrons in the Lewis structure of CH3OH.
14
Among those combinations, which leads to the ionic compound having the largest lattice energy?
A-Y
Which combinations of these ions produce ionic compounds where there is a 1:1 ratio of cations and anions?
B-X and A-Y
Cr2+ ions are represented by the electron configuration ________.
[Ar]3d4
Using the noble gas shorthand notation, write the electron configuration for Fe3+.
[Ar]3d^5
What is the electron configuration for the Fe2+ ion?
[Ar]4s03d6
What is the electron configuration of an atom of this element? (Ru)
[Kr]4d^75s^1
The electron configuration of the P3- ion is ________.
[Ne]3s23p6
The electron configuration of the sulfide ion (S2-) is ________.
[Ne]3s23p6
In which of the molecules below is the carbon-carbon distance the shortest? a. H-C≡≡C-H b. H3C-CH2-CH3 c. H2C=C=CH2 d. H2C=CH2 e. H3C-CH3
a
In the nitrite ion (NO2-), ________.
both bonds are the same
Which halogen, bromine or iodine, will form the more polar bond with phosphorus?
bromine
A substance XY, formed from two different elements, boils at -33 ∘C. Is XY likely to be a covalent or an ionic substance?
covalent
Phosphorus pentchloride (PCl5) is used as a chlorinating reagent in chlorination of organic compounds. What type of bonding occurs between the atoms of a PCl5 molecule?
covalent
Of the bonds below, ________ is the most polar. a. Si-Cl b. P-S c. Na-S d. Na-Cl e. C-F
d. Na-Cl
Which two would be likely to form a compound of formula XY2? a. PI2 b. BO2 c. PO2 d. TeI2
d. TeI2
For a given arrangement of ions, the lattice energy increases as ionic radius ________ and as ionic charge ________.
decrease, increases
As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________.
decreases, increases
Which of the following has the bonds correctly arranged in order of increasing polarity? a. O - F, Be - F, Mg - F, N - F b. Mg - F, Be - F, N - F, O - F c. N - F, Be - F, Mg - F, O - F d. Be - F, Mg - F, N - F, O - F e. O - F, N - F, Be - F, Mg - F
e. O - F, N - F, Be - F, Mg - F
Which of the following has eight valence electrons? a. Ti4+ b. Cl- c. Na+ d. Kr e. all of the above
e. all of the above
The Lewis structure of N2H2 shows ________.
each nitrogen has one nonbonding electron pair
The ability of an atom in a molecule to attract electrons is best quantified by the ________.
electronegativity
What is the trend in electronegativity going from left to right in a row of the periodic table?
electronegativity increases going from left to right in a row
methane reacts with chlorine to make methyl chloride. Is this reaction exothermic or endothermic? is delta H positive or negative?
exothermic, negative
T or F: Atoms surrounded by eight valence electrons tend to lose electrons.
false
T or F: Compounds in which nitrogen is the central atom are frequent exceptions to the octet rule because they have too many electrons surrounding the nitrogen
false
T or F: The Si in SiH4 does not follow the octet rule because hydrogen is in an unusual oxidation state.
false
T or F: When a metal loses an electron, the process is exothermic.
false
True or false: An element's number of valence electrons is the same as its atomic number.
false
Phosphorus oxychloride has the chemical formula POCl3POCl3, with PP as the central atom. In order to minimize formal charge, how many bonds does phosphorus make to the other atoms in the molecule? (Count each single bond as one, each double bond as two, and each triple bond as three).
five
In the correct Lewis structure for the nitrate ion, NO3 -, nitrogen has how many covalent bonds?
four
Most explosives are compounds that decompose rapidly to produce ________ products and a great deal of ________.
gaseous, heat
State whether the bonding in each compound is likely to be covalent or not: argon, sodium chloride, water, oxygen, iron
no, no, yes, yes, no
Which of the following is the best Lewis symbol for iodine?
o o o | o | o o o
The type of compound that is most likely to contain a covalent bond is ________.
one that is composed of only nonmetals
To convert from one resonance structure to another, ________.
only electrons can be moved
Which of the following is the best Lewis symbol for oxygen?
oo o O o oo
