exam 3 review questions Flashcards
The ground state electron configuration for Zn is?
[Ar]4s^23d^10
The element that has the valance configuration of 2s^1 is?
Li
In which set of elements would all members be expected to have the most similar properties?
K,Rb, Cs (down a row)
The effective nuclear charge of an atom is determined by the?
the nuclear charge and number of core electrons.
the atomic radius of main-group elements generally decreases from left to right across a period because?
Effective nuclear charge increases from left to right
Which ionic compound has the smallest ionic separation?
LiF
Of the groups listed, which have the lowest first ionization energies?
Alkaline earth metals
The electron affinity of oxygen is represented by which equation?
O (g) + e^- ā> O^- (g)
Which of the listed oxides is the most acidic?
P4O6
Which one of the following is true about alkali metals?
They are readily form ions with a +1 charge.
All of the following reactions concerning alkali metals are correct except?
Na(s) + H2(g) ā> NaH2 (s)
Alkaline earth metals tend to be less reactive than alkali metals because alkaline earth metals have?
higher ionization energies
The allotrope of oxygen that is important for absorbing ultraviolet light in the stratosphere is?
O3
Element X reacts with oxygen to form an oxide with the formula X2O. When X2O is dissolved in water, the resulting solution is basic. Element X could be
potassium
The numbers of valence electrons in the alkali metals, the alkaline earth metals, and the halogens are _____ respectively.
1,2 and 7
For ionic compounds as the ionic radius decreases the lattice energy generally
increases if the ionic charges are the same
Which ion does not have a closed shell noble gas configuration
S^2+
What is the principal quantum number of the valance electrons in atomic calcium?
4
In which of the molecules below is the nitrogen-nitrogen distance expected to be the shortest?
NāN (Tripple Bond)
A triple bond consists of __ electrons shared between two atoms
6
How many single covalent bonds must a sulfur atom form to have a complete octet in its valance shell?
2
Ionization energies generally __ from left to right within a period and __ from top to bottom within a group
increase, decrease
____ describes the ability of an atom in a molecule to attract electrons
electronegativity
How many valence electrons does the species SF6 have?
48
What is the formal charge on nitrogen NO-2
0
How many equivalent resonance forms can be drawn for the nitrite ion?
2
The central atom in ___ is hypervalent
SF6
The electron-domain geometry of the central atom in the following is tetrahedral except for which one?
NO-3
The molecular geometry of the PF3 molecules is
trigonal pyramidal
Using the VSEPR model, the molecular geometry of CIF5 is
square pyramidal
Which of the following molecules would be considered nonpolar?
CO2
The sp atomic hybrid orbital set accommodates __ electron domains
2
The hybridization of the central atom in SiH4 and PH3 are __ and __
sp^3, sp^3
The hybridization of carbon in the H-C(triple)C-H molecule is
sp
The angles between sp^2 orbitals are?
120
There are __ sigma and __ pi bonds in the H2C(triple)CH2 molecule
5,1
Mixing one s atomic orbital and one p atomic orbital gives rise to
two sp hybrid orbitals
In a typical C(triple)C double bond, the sigma bond results from the overlap of __ orbitals, and the pi bonds result from the overlap of __ orbitals.
sp^2 hybrid, p-atomic
Based on molecular orbital theory, the bond order of the bond in the H2+ ion is
0
