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WorksheetsAP Chem Unit 1
Total questions: 83
Worksheet time: 2hrs 1mins
According to the information in the table here, a 1.00 g sample of which of the following contains the greatest mass of oxygen?
Na2O
MgO
K2O
CaO
The average atomic mass of a newly discovered element is 10.600 amu. It has two naturally occurring isotopes. One has a mass of 10.000 and a natural abundance of 70.000%. What is the isotopic mass of the other isotope?
10.000
9.0000
12.000
11.000
A new element has two isotopes, one with a mass of 40.0 amu that is 75% abundant. The average atomic weight of the element is 40.50 amu. What is the isotopic mass of the other isotope?
40.0 amu
42.0 amu
41.0 amu
44.0 amu
108 g of an element Z reacts with oxygen to form 204 g of the oxide Z2O3. What is the element Z?
Al
Sc
Ag
Mn
Which contains the largest number of atoms?
3.0 mL of CH3OH (density = 1.2g/mL)
3.0 moles of CO
3.0 mg of water
3.0x1022 molecules of nitrogen gas
Estimate the number of moles of hydrogen in 176g of pentanol, C5H11OH. The molar mass of pentanol is 88g/mol.
12 mol H
144 mol H
24 mol H
72 mol H
An Olympic medal contains 71.5% of gold by mass. How much gold could be extracted from a medal that weighs 115 grams?
0.417 mol
1.33 mol
0.817 mol
14.1 mol
How would you be able to separate the hydrogen from the oxygen in water?
by using a filter
distillation
electolysis (using electricity)
by using tweezers
If matter is not uniform throughout and can be separated by physical means it is a ________.
a compound
an element
a heterogeneous mixture
a homogeneous mixture
What is the element?
Mass Number = 197
Number of Electrons = 79
Number of Neutrons = 118
Copper
Boron
Silver
Tin
What is the mass number of this element?
17
18
35
7
An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.
+2
-2
+3
0
How do you write the balanced equation of burned propane (C3H8) in the presence of oxygen to produce water and carbon dioxide?
C3H8 + O2 → H2O + CO2
C3H8 + O2 → 4H2O + 3CO2
C3H8 + 5O2 → 4H2O + 3CO2
C3H8 + 3O2 → 2H2O + 3CO2
The blue elements (left side) are called
Write the formula for the following: Hydroiodic Acid
(a)
Find the molar masses of the following compounds:
(NH4)2CO3
303.3 g/mole
102.9 g/mole
74.1 g/mole
160.0 g/mole
96.0 g/mole
Find the percent composition of both Copper and Sulfur in the compound Cu2S?
%Cu= 67.987 %S= 32.013
%Cu= 79.854 %S= 20.145
%Cu= 35.946 %S= 64.054
In a reaction, 9 grams of a substance are produced. The theoretical yield was 10 grams. What is the percentage yield?
80%
85%
90%
95%
Mg + 2HCl --> MgCl2 + H2
SO2 + PCl5 ⟶ SOCl2 + POCl3
What mass of SOCl2 is produced when 16.2g SO2 react with 13.7g PCl5?
Quinone, which is used in the dye industry and in photography, is an organic compound containing only C, H, and O. What is the empirical formula of the compound if you find that 0.105 g of the compound gives 0.257 g of CO2 and 0.0350 g of H2O when burned completely?
CHO
C2H10
C6H4O2
C3H2O
The simplest formula for an oxide of element Z (MM= 86.0) that is 32% oxygen by weight is
Z2O
ZO2
Z2O5
ZO
When reading a PES graph, the higher the peak, _______________
the more energy the electrons contain
the more electrons are in that sublevel
the further the electrons are from the nucleus
the higher the first ionization energy
When reading a PES graph, a larger binding energy means
there are more electrons in that sublevel
the closer the electrons are to the nucleus
the lower the ionization energy
the further away the electrons are from the nucleus
What is the electron configuration for the zinc atom in the ground state?
1s2 2s2 2p6 3s2 3p6 4s2 3d10
1s2 2s2 2p6 3s2 3p6 4s2 4d10
1s2 2s2 2p6 3s2 3p6 4d10
1s2 2s2 2p6 3s2 3p6 3d10
What is the electron configuration for the zinc ion?
1s2 2s2 2p6 3s2 3p6 3d10
1s2 2s2 2p6 3s2 3p6 4s2 3d8
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
1s2 2s2 2p6 3s2 3p6 4d10
In a PES graph, 1s electrons will have a _______ binding energy than 2s electrons.
higher
lower
same
When Ca becomes an ion, it _______ electrons and gets _________.
loses
smaller
loses
larger
gains
smaller
gains
larger
What element is represented by this mass spectroscopy graph?
B
C
Na
Be
Ne
How many isotopes does this mass spectroscopy graph represent?
(a)
How many neutrons does the most abundant isotope have on this mass spectroscopy graph?
24
25
26
12
13
Write the ionic formula for sodium acetate
NaC2H3O2
Na2C2H3O2
Na(C2H3O2)2
C2H3O2Na
C2H3O2Na2
Write the ionic formula for tin(II) chloride
SnCl2
Sn2ClO2
SnCl
Sn2Cl
SnCl4
Write the ionic compound for calcium hydroxide
Ca(OH)2
CaOH
CaO
Ca2OH
CaH2
Write the ionic compound for zinc sulfate
ZnSO4
not enough info
Zn2SO4
Zn(SO4)2
ZnSO3
Write the ionic compound for ammonium sulfate
(NH4)2SO4
NH4SO4
NH3SO4
(NH4)2SO3
(NH3)2SO3
Write the ionic compound for manganese(II) chloride
(a)
Write the ionic compound for copper(I) nitrate
(a)
Write the ionic compound for silver chloride
(a)
Write the ionic formula for lead(II) nitrate
(a)
Write the ionic compound for sodium iodide
(a)
Write the ionic formula for lithium fluoride
(a)
Write the name for K2S
potassium sulfide
potassium sulfate
dipotassium sulfide
potassium(II) sulfide
Match an ionic formula with each name:
lead(II) nitrate = (a)
lead(II) nitrite = (b)
lead(IV) nitride = (c)
Metals (a) electrons in order to acquire a full octet.
Non-metals (b) electrons in order to acquire a full octet.
Organize these options by charge the element makes as an ion:
Na
Mg
F
O
K
Ca
Br
Se
Group 1A
Group 2A
Group 7A
Group 6A
Cations
Gain electrons, has an overall positive charge
Lose electrons, has an overall positive charge
Lose electrons, has an overall negative charge
Gain electrons, has an overall negative charge
Write the formula for the binary ionic compound: aluminum sulfide.
(a)
Write the formula for the binary ionic compound: magnesium iodide.
(a)
Write the formula for the ternary ionic compound: strontium chlorate.
(a)
The proper formula for magnesium hydroxide.
MgOH
Mg2OH
Mg(OH)2
Mg2OH2
Which of the following is NOT an ionic compound:
NaCl
Cl2
CaF2
KOH
K forms the compound K2O, which is an ionic compound that is brittle. Identify another element, M, that is likely to form a brittle compound with the formula M2O.
Na2O because Na is in the same group as K therefore they have the same # of valence electrons
Ca2O because Ca is in the same row as K, therefore they have similar properties
Ba2O because Ba is in the same row as K, therefore they have the same # of valence electrons
Zn2O because Zn is in the same row as K, therefore they have similar properties
Rb2O because Rb is in the same group as K therefore has more energy shells which creates brittle compounds
Cl forms the compound MgCl2, which is a white crystalline solid with a high melting point. Identify another element, X, that is likely to form a white crystalline solid with a high melting point with the formula MgX2.
MgF2 because F is in the same family as Cl therefore they have the same # of valence electrons
MgS2 because S is in the same row as Cl, therefore they have similar properties
MgSi2 because Si is in the same row as Cl, therefore they have the same # of valence electrons
MgNa2 because Na is also a metal and metallic solids have high melting points.
MgBr2 because Br is in the same group as Cl therefore has more energy shells which creates crystalline solids
How many moles is 100.0 grams of the ionic compound formed between sodium and sulfur?
Round to 3 significant digits and don't include units
(a)
What is the molar mass of the ionic compound formed between calcium and phosphate?
Round to a whole number
(a)
How many grams is 1.30 moles of the ionic compound formed from zinc and nitrate?
Round to 3 significant figures
(a)
The table here shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend?
The atomic radius of oxygen is greater than the atomic radius of fluorine
The atomic radius of oxygen is less than the atomic radius of nitrogen
There is repulsion between paired electrons in oxygen's 2p orbitals
There is attraction between paired electrons in oxygen's 2p orbitals
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 more electrons than O2- has.
F- is more electronegative than O2- is.
For element X represented here, which of the following is the most likely explanation for the large difference between the second and third ionization energies?
The effective nuclear charge decreases with successive ionizations.
The shielding of outer electrons increases with successive ionizations.
The electron removed during the third ionization is, on average, much closer to the nucleus than the first two electrons removed were.
The ionic radius increases with successive ionizations.
Which of the following correctly compares periodic properties of two elements and provides an accurate explanation for that difference?
The first ionization energy of Al is greater than that of B because Al has a larger nuclear charge than B does.
The first ionization energy of F is greater than that of O because O has a higher electronegativity than F has.
The atomic radius of Ca is larger than that of Mg because the valence electrons in Mg experience more shielding than the valence electrons in Ca do.
The atomic radius of Cl is smaller than that of S because Cl has a larger nuclear charge than S does.
Based on the ionization energies of element X given in the table here, which of the following is most likely the formula of the compound formed between element X and SO42-?
XSO4
X2SO4
X2(SO4)3
X(SO4)2
Which of the following best helps to explain why the electron affinity of Br has a greater magnitude than that of I?
Br has a lower electronegativity than I does.
Br has a lower ionization energy than I does.
An added electron would go into a new shell in Br but not in I.
There is greater attraction between an added electron and the nucleus in Br than in I.
Choose the one that has the highest electronegativity
Cs
Pb
Br
Se
Choose the one that has the largest atomic radius
Cs
Pb
Br
Se
Choose the one that has the lowest first-ionization energy
Cs
Pb
Br
Se
Given that the density of Hg(l) at 0oC is about 14 g/mL, which of the following is closest to the volume of one mole of Hg(l) at this temperature?
0.07 mL
0.14 mL
1.4 mL
14 mL
Given that the density of Tl(l) at 0oC is about 11.85 g/mL, which of the following is closest to the volume of one mole of Tl(l) at this temperature?
0.084 mL
0.17 mL
1.7 mL
17 mL
A student has a 1 g sample of each of the following compounds:
NaCl, KBr, and KCl.
Which of the following lists the samples in order of increasing number of moles in the sample?
NaCl < KCl < KBr
NaCl < KBr < KCl
KCl < NaCl < KBr
KBr < KCl < NaCl
A student obtains a sample of a pure solid compound. In addition to Avogadro's number, which of the following must the student know in order to determine how many molecules are in the sample?
Mass of the sample, volume of the sample
Mass of the sample, density of the sample
Molar mass of the compound, mass of the sample
Molar mass of the compound, density of the sample
A solution of methanol, CH3OH, in water is prepared by mixing together 128 g of methanol and 108 g of water. The mole fraction of methanol in the solution is closest to:
0.80
0.60
0.50
0.40
A solution is prepared by adding 16 g of CH3OH (molar mass 32 g) to 90 g of H2O (molar mass 18 g). The mole fraction of CH3OH in this solution is closest to which of the following?
0.1
0.2
0.3
0.4
In 1.00 mol of potassium zirconium sulfate trihydrate, K4Zr(SO4)4 * 3 H2O, there are:
4 x 6.02 x 1023 potassium atoms
3 x 6.02 x 1023 hydrogen atoms
6.02 x 1023 sulfur atoms
4 moles of zirconium atoms
How many carbon atoms are contained in 2.8 g of C2H4?
1.2 x 1023
3.0 x 1023
6.0 x 1023
1.2 x 1024
How many hydrogen atoms are contained in 2.8 g of C2H4?
1.2 x 1023
2.4 x 1023
6.0 x 1023
1.2 x 1024
A 100.0 g sample of which of the following compounds contains the most molecules?
CO2
SO2
H2O
N2O
Which of the following numerical expressions gives the number of particles in 2.0 g of Ne?
