Chemistry Final Chapter Eight
The central atom in ________ does not violate the octet rule.
CF4
The ________ ion has a noble gas electron configuration.
Cl-
In which of the molecules below is the carbon-carbon distance the shortest?
H-C---C-H
The only noble gas without eight valence electrons is ________.
He
Elements from opposite sides of the periodic table tend to form ________.
Ionic compounds
Resonance structures differ by ________.
Placement of electrons only
A ________ covalent bond between the same two atoms is the longest.
Single
Based on the octet rule, aluminum most likely forms a ________ ion.
Al3+
Of the atoms below, ________ is the least electronegative.
B
Of the following, ________ cannot accommodate more than an octet of electrons.
Be
Of the atoms below, ________ is the most electronegative.
C
Lattice energy is ________.
The energy required to convert a mole of ionic solid into its constituent ions in the gas phase
The Lewis structure of the CO32- ion is ________.
[:O:=C-::O:-::O:]2-
Which of the following noble gas electron configurations represents the Ru+ cation?
[Kr]5s14d6
Of the possible bonds between carbon atoms (single, double, and triple), ________.
a double bond is longer than a triple bond
Bond enthalpy is ________.
always positive
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
The Lewis structure of N2H2 shows ________.
each nitrogen has one nonbinding electron pair
A nonpolar bond will form between two ________ atoms of ________ electronegativity.
identical, equal
Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.
increases, decreases
The type of compound that is most likely to contain a covalent bond is ________.
one that is composed of only nonmetals
Of the bonds C-C, C C, and C≡C, the C-C bond is ________.
weakest/longest
What is the maximum number of double bonds that a carbon atom can form?
2
How many different types of resonance structures can be drawn for the ion SO32-?
3
How many equivalent resonance forms can be drawn for CO32-? (Carbon is the central atom.)
3
How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?
4
What is the principal quantum number of the last shell for the element barium?
6
The formal charge on nitrogen in NO3- is ________, where the Lewis structure of the ion is:
+1
In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________.
0,0
In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________.
1+
The Lewis structure of PF3 shows that the central phosphorus atom has ________ nonbonding and ________ bonding electron pair(s).
1, 3
The ability of an atom in a molecule to attract electrons is best quantified by the ________.
Electronegativity
In the molecule below, which atom has the largest partial negative charge? Cl | F— C —Br | I
F
Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br
O, Se
Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5
O-H
