WorksheetsAP Chem Unit 1 & 2 Review
Total questions: 28
Worksheet time: 14mins
A compound contains 1.00 mol of Sb. 1.50 mol C and 4.50 mol of O What is the empirical formula?
SbCO
Sb2C3O9
SbC1.5O4.5
SbC3O9
Based on this mass spectrum, how many isotopes does Mercury have?
1
3
5
7
What is the molar mass for Na2O to 4 sig. figs. Do not include units.
(a)
What is the molar mass of HgHCO3
229.61 g/mol
287.65 g/mol
378.40 g/mol
261.6 g/mole
Which of the following nickle compounds contains the highest percentage nickle by mass?
NiCl2
NiO2
NiO
Ni3(PO4)2
A compound has the molecular formula of PBr5, it has a molecular formula mass of 431 g/mol. What is the molecular formula of this compound?
P2Br10
PBr5
P3Br15
P4Br20
Select all of the empirical formulas from this list.
CH2
C3H6
C5H10P
Na2O2
C4H8P2
For the compound whose formulas is C4H8P2, enter the mass % for Hydrogen, to 3 Sig. Figs. Enter just a number for your answer.
(a)
What is the mass of Na2CO3⋅7H2O
105.99 g/mol
741.963 g/mol
232.13 g/mol
1183.07 g/mol
The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electrons of Ne. This difference best accounts for which of the following statements.
Na has a higher melting point than Ne.
Na has a lower first ionization energy than Ne.
Na has fewer naturally occurring isotopes than Ne.
Na has a higher neutron-to-proton ratio than Ne.
The elements in which of the following groups have most nearly the same atomic radius?
Mg, Ca, Sr, Ba
C, P, Se, I
Cr, Mn, Fe, Co
Ne, Ar, Kr, Xe
What element is this the orbital diagram and electron configuration for?
Potassium
Aluminum
Neon
Argon
The ionization energies for element X are listed in the table. On the basis of the data, element X is most likely
Na
Mg
Al
Si
Which of the following best helps to account for the fact that the F⁻ ion is smaller than the O²⁻ ion?
F⁻ has a larger nuclear mass than O²⁻ has
F⁻ has a larger nuclear charge than O²⁻ has
F⁻ has a electrons than O²⁻ has
F⁻ is more electronegative than O²⁻ is
Which of the following best explains the deviation of the 1st IE of Oxygen from the over all trend in the table
The atomic radius of O is greater than the atomic radius of F.
The atomic radius of O is less than the atomic radius of N.
There is repulsion between paired electrons in O's 2p orbitals.
There is attraction between paired electrons in O's 2p orbitals.
Determine the electron configuration for N3-
1s22s22p5
1s22s22p6
1s22s22p3
1s22s2
Which of the following is the most electronegative element?
O
La
Rb
Mg
N
How many valance electrons are seen in this PES?
2
4
6
8
Which of the following are covalent compounds?
Zn2+
CH2O
NH4+
NaI
F2
Which of the following bonds will be most polar?
Si-O
C-H
O-O
B-F
Which of the following best explains why copper conducts electricity?
It can have two or three valence electrons
It has delocalized electrons that can flow in a circuit
It is a transition metal
It has a low electronegativity
Does this model represent an ionic compound? Why or why not?
What is a substitutional alloy?
A metal with one element
A metal with two elements of similar size
A metal with two elements of very different sizes
A metal with layers of different elements
Which is the correct Lewis structure for the compound CH2O?
What hybridization exists for the compound CH2O?
sp3
sp2
sp
there is no hybridization
A resonance structure for CH2O is shown in the picture. Why is this not the best resonance structure?
because the carbon only has 6 valence electrons
because the oxygen doesn't have a full octet
because the formal charges of oxygen and carbon aren't equal to zero
because the hydrogens don't have a full octet
Which of the following types of bonding results in materials which have the highest melting and boiling points?
ionic bonding
metallic bonding
covalent bonding
Which color graph would be the plot for the molecule with the shortest bond length?
purple graph
blue graph
red graph
