AP Chem Summer Assignment Worksheet #1
Atomic Structure
1. a) For the ion
39 +
19
K , state how many electrons, how many protons, and how many
neutrons are present?__________________________________________________________
b) Which of these particles has the smallest mass?
____________________________________________________________________________
2. An atom has a net charge of -1.it has 18 electrons and 20 neutrons. Give a) its isotopic symbol b)
its atomic number c) the charge on its nucleus d) the number of protons.
a)_____________________________________________
b)______________________________________________
c)_____________________________________________
d)______________________________________________
3. What is the number of electrons in
87
37
Rb+?
______________________________
4. Determine the number of protons, electrons, and neutrons in
80
Br- and
35
79
34
Se ?
________________________________________________________________________________________________________________________
5. Complete the following table.
Symbol
90
…
Sr+2
Na…
….
Br…
Atomic
number
Mass
number
11
35
82
# of
protons
38
# of
electrons
# of
neutrons
10
12
Net
charge
1-
6. Complete the following table.
Isotopic
Symbol
# of protons
# of neutrons
13
6
7
Cl
17
18
Fe
26
56
1
3
C
….
H
70
Sn
Atomic mass#
120
7. Which of the following statements is wrong for structure of an atom?
A) Protons and neutrons are in the center.
B) Electrons are moving around the nucleus.
C) Electrons are negatively charged particle.
D) Neutrons are positively charged particles.
E) Mass of one proton is equal to mass of one neutron.
8. Which of the following statements is (are) true for structure of an atom?
I. Volume of a nucleus is smaller than volume of its atom.
II. The atomic mass number is the sum of proton and neutron numbers.
III. The atomic number is the sum of protons and electrons.
A) I
B) II
C) III
D) I , II
E) I, II , III
9. 1) Proton number 2) Neutron number 3) Chemical properties 4) Physical properties
Which of the above is (are) different for isotopes?
A) II
B) III
C) I , IV
D) II , III
E) II , IV
10. If X+2 has 28 electrons and 35 neutrons, what is the atomic mass number of X?
A) 68
B) 67
C) 65
11. If atomic mass number of
A) 27
B) 24
24X
C) 51
D) 63
E) 60
is 51, what is the number of neutrons of X?
D) 75
E) 40
12. If X+2 has 28 electrons and 35 neutrons, what is the atomic mass number of X?
A) 68
B) 67
C) 65
13. If atomic mass number of
A) 27
B) 24
D) 63
24X
is 51, what is the number of neutrons of X?
C) 51
D) 7 5
14) What is the atomic mass number of
236
92U?
a) 92
d) 328
b) 144
c) 236
15) What is the neutron number of
a) 92
b) 144
E) 60
E) 40
236
92U?
c) 236
d) 328
16. The element F has 10 neutrons and a mass number = 19. How many electrons are in its outermost shell?
A) 10
B) 3
C) 9
D) 7
17. Which one is a stable isotope of
A)
17
34
X
B)
18
33
X
C)
19
37
17
X
35
E) cannot tell from the information given
Cl.
D)
20
36
X
18. The most common form of iron has 26 protons and 30 neutrons in its nucleus. State its atomic
number, atomic mass, and number of electrons if it's electrically neutral.
Atomic number: _______ Atomic mass: ________ # of electrons: __________
19. Consider the following three atoms: Atom 1 has 7 protons and 8 neutrons; atom 2 has 8 protons
and 7 neutrons; atom 3 has 8 protons and 8 neutrons. Which two are isotopes of the same element?
____________________
20. Consider fluorine atoms with 9 protons and 10 neutrons. What are the atomic number and
atomic mass of this fluorine? Suppose we could add a proton to this fluorine nucleus. Would the
result still be fluorine? Explain. What if we added a neutron to the fluorine nucleus?
Atomic number: ____________
Atomic mass: _____________
21. How many neutrons are in the nucleus of an atom of tungsten-184 which has an atomic number
of 74?
# of neutrons:_________________
22. Which of the following combinations of particles represents an ion of net charge -1 and of mass
number 82?
(A) 46 neutrons, 35 protons, 36 electrons
(C) 46 neutrons, 36 protons, 36 electrons
(E) 47 neutrons, 35 protons, 36 electrons
(B) 46 neutrons, 36 protons, 35 electrons
(D) 47 neutrons, 35 protons, 35 electrons
23. One species of element M has an atomic number of 10 and a mass number of 20; one species of
element N has an atomic number of 11 and a mass number of 20. Which of the following statements
about these two species is true?
(A) They are isotopes.
(B) They are isomers.
(C) They are isoelectronic
(D) They contain the same number of neutrons in their atoms.
(E) They contain the same total number of protons plus neutrons in their atoms.
24. A neutral atom has an atomic number of 30 and a mass number of 62, the atom must contain:
(A) 92 neutrons
(C) 29 neutrons
(B) 62 electrons
(D) 30 electrons
25. Atom X has 12 protons, 12 electrons, and 13 neutrons. Atom Y has 10 protons, 10 electrons, and
15 neutrons. It can therefore be concluded that:
(A) atoms X and Y are isotopes.
(C) atoms X and Y have the same mass number.
(B) atom X is more massive than atom Y.
(D) atoms X and Y have the same atomic number.
26. A neutral atom which has 42 electrons and a mass number of 93 has
(A) an atomic number of 51.
(C) a nucleus containing 40 neutrons.
(B) a nucleus containing 51 neutrons.
(D) a nucleus containing 51 protons.
27. A sodium ion, Na+, contains the same number of electrons as
(A) a sodium atom, Na.
(C) a potassium ion, K+.
(B) a magnesium atom, Mg.
(D) a neon atom, Ne.
AP Chem Summer Assignment Worksheet #2
Electronic Configuration
Write the electron configurations using arrows of the following elements:
1)
Magnesium
_________________________________________________
2) Cobalt
__________________________________________________
3) Krypton
___________________________________________________
4) Beryllium
___________________________________________________
5) Scandium
___________________________________________________
Write the electron configurations of the following elements:
6)
Nickel
______________________________________________________
7)
Cadmium______________________________________________________
8)
Selenium ______________________________________________________
9)
Strontium______________________________________________________
10)
Lithium ______________________________________________________
Determine what elements are denoted by the following electron configurations:
11)
1s22s22p63s23p5 ____________________
12)
1s22s22p63s23p64s23d104p65s2 _____________________
13)
[Kr] 5s24d105p4 ___________________
14)
[Xe] 6s24f145d7 ___________________
15)
[Rn] 7s25f12 ___________________
Determine whether the following electron configurations are or are not valid:
16)
1s22s22p63s23p64s24d104p6
17)
1s22s22p63s33d6
18)
[Rn] 7s25f9
__________________
19)
[Xe]
__________________
20)
[Ne] 3p5 3s2
__________________
_________________
__________________
AP Chem Summer Assignment Worksheet #3
Periodic Table
1. A gaseous ion X2+ has two unpaired electrons in its most stable state. If X is a representative
element, to which groups could the element X belong?
a) IA and VIA
b) IVA
c) VA and VIIA
d) IA and IIIA
e) VIA and VIIA
2. In the fourth period of the Periodic Table, how many elements have one or more 4p electrons?
a) 2
b) 6
c) 10
d) 18
d) 32
3. A horizontal row in the periodic table containing a sequence of elements is a:
a) Group
b) family
c) subgroup
d) period
4. The modern periodic table has the elements arranged in order of:
a)
b)
c)
d)
e)
their date of discovery.
increasing radii of the atoms.
increasing number of neutrons.
increasing number of protons.
number of isotopes.
5. Which of the following electron configurations is correct for chromium, (atomic number 24)?
a)
b)
c)
d)
e)
[Ar]4s24p4
[Ar]3d54s1
[Ar]3d45s2
[Kr]4d55s1
[Ar]4s14p5
6. The electron configuration of Pt is [Xe]4f145d96s1. How many unpaired electrons are in this atom?
a) 1
b) 2
c) 7
d) 8
7. Which of the following statements is false?
a)
b)
c)
d)
e)
The s orbital is spherical.
There are 10 d orbitals in a d subshell.
The third energy level has no f orbitals.
The fifth energy level has a set of f orbitals.
A set of p orbitals can have a maximum of 6 electrons.
e) 9
8. For a group in the periodic table, the elements have in common:
a)
b)
c)
d)
e)
the
the
the
the
the
same
same
same
same
same
number
number
number
number
number
of
of
of
of
of
electrons.
electrons in all subshells.
filled subshells.
electrons in the highest energy subshell containing electrons.
orbitals.
9. Which of the following electron configurations belong to an element
that is the most chemically reactive?
a) 1s2
b) 1s2 2s2 2p6
c) 1s22s22p5
(d) 1s22s22p63s23p6
10. How many valence electrons does the element with the electron configuration 1s22s22p63s23s64s1 have?
a. 0
b) 1
c) 9
d) 19
11. How is the electron configuration similar for each element in a group?
___________________
12. How is the electron configuration similar for each element in a period?
___________________
13. Refer to a periodic table. In which period is calcium?
a. Period 2
b. Period 4
c. Period 6
d. Period 8
14. Refer to a periodic table. In which group is calcium?
a. Group 1
b. Group 2
c. Group 17
d. Group 18
15. An element that has the electron configuration [Ne]3s23p5 is in which period?
a. Period 2
b. Period 3
c. Period 5
d. Period 7
16. An element that has the electron configuration [Ne]3s23p5 is in which group?
a. Group 2
b. Group 5
c. Group 7
d. Group 17
AP Chem Summer Assignment Worksheet #4
Mole Concept
Complete the following problems showing all work and with answers using the correct
significant digits.
1)
How many grams does 0.500 moles of NaCl weigh?
____________________
2)
How many molecules are there in 0.655 moles of C6H14?
____________________
3)
How many moles are there in 1.204 x 1025 molecules of water?
____________________
4)
How many grams does2.408 x 1023 molecules of SiO2 weigh?
____________________
5)
How many molecules are there in 21.6 grams of CH4?
____________________
6) Calculate the molecular mass for the following:
A. KOH
______________
B. N2O2
___________________
C. Cu2SO3
______________
D. Sr3 (PO4)2_________________
7) Convert each of the following from grams to moles.
A. 15.O g C2H6
_________________
B. 36 g H2O ____________________
C. 80 g NaOH__________________
D. 50 g CaCO3___________________________
8) Convert moles to grams in each of the following:
A. 2 mole NH3_____________________________
B. 0.5 mole H2SO4_____________________________
9) Convert the following to moles:
A. 3.01 X 1023 atoms Na ____________________
B. 6.02 X 1024 molecules CO2 _____________________
10) Calculate the molecular mass of the following compounds:
a. acetone, CH3COCH3 _________________________
b. ethyl ether, C4H10 ____________________________
11) How many moles of hydrogen atoms are there in 1 mole of following molecules?
a. C3H8____________________
b. C2H5OH_____________________________
12) How many moles of atoms are there in 2 moles of following molecules?
a. C10H22 ___________________
b. CH3COOH__________________________
AP Chem Summer Assignment Worksheet #5
Chemical Formula /Percent Composition
Complete the following problems showing all work and with answers using the correct
significant digits.
1. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting
oxide weighed 1.560 grams. Determine the percent composition of each element in the
compound.
___________________
2. Determine the empirical formula given the following data for each compound: (a) Fe =
63.53%, S = 36.47% (b) Fe = 46.55%, S = 53.45%
(a)___________________(b)______________
3. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the
empirical formula of the compound.
__________________
4. A 2.500 gram sample of uranium was heated in air. The resulting oxide weighed 2.949
gram. Determine the empirical formula of the oxide. {Hint: Carry out the calculations to four
decimal places}.
__________________
5. When 1.010 g of zinc vapor is burned in air, 1.257 grams of the oxide is produced.
a) What elements are present in the oxide?
b) Determine the percent composition of each element in the oxide.
c) Determine the empirical formula of the compound.
(a)_________________ (b)________________ (c)_______________
6. A compound has the empirical formula of CH3Br and a vapor density of 6.00 g/L, at 375
K and 0.983 atm. Using these data, determine the following:
a) The molar mass of the compound.
b) The molecular formula of the compound.
(a)________________ (b)_______________
7. A compound containing the elements C, H, N, and O is analyzed. When a 1.2359 gram is
burned in excess oxygen, 2.241 g of CO2 (g) is formed. The combustion analysis showed that
the sample contained 0.0648 g of H.
a) Determine the mass, in grams, of C in the 1.2359 g sample of the compound.
b) When the compound is analyzed for N content only, the mass percent of N is
found to be 28.84%. Determine the mass, in grams, of N in the original 1.2359 g
sample of compound.
c) Determine the mass, in grams, of O in the original 1.2359 g sample of the
compound.
d) Determine the empirical formula of the compound.
(a)_________________ (b)__________________ (c)_________________ (d)______________
AP Chem Summer Assignment Worksheet #6
Stoichiometry
Balance all of the equations that need to be balanced. The answers are given in
parenthesis at the end of each problem.
1. In the decomposition of sodium hydroxide, how many moles of sodium
hydroxide are needed to produce 30.0 moles of water? (60.0 moles NaOH)
__________________
2. In the single replacement reaction of lithium and magnesium nitrate, what
mass of lithium combines with 75.0 grams of magnesium nitrate? (7.02 g Li)
_________________
3. How many grams of lead (II) nitrate are needed to produce 60.0 grams of
potassium nitrate in the double replacement reaction of potassium iodide and
lead (II) nitrate. (98.3 g lead (II) nitrate)
_________________
4. In the synthesis reaction of zinc(II) and sulfur, what mass of zinc (II) sulfide
is produced from 100.0 grams of sulfur? (303.9 g ZnS)
________________
5. A synthesis reaction of calcium and oxygen was completed in a lab and
234.9 grams of calcium oxide were produced from 75.00 grams of oxygen.
What is the percent yield? (89.36%)
_______________
6. In the single replacement reaction of magnesium and aluminum phosphate,
if 7.00 moles of magnesium react, how many moles of aluminum phosphate
would be needed? (4.67 mol AlPO4)
_______________
7. When methane and oxygen react (complete combustion reaction) how many
grams of water would be produced from 25.0 grams of methane? (56.1g water)
_______________
8. A 26.3 gram sample of potassium chlorate decomposed and produced 9.45
grams of oxygen. What is the percent yield for oxygen? (91.7%)
______________
9. If 7.40 grams of calcium hydroxide react with nitric acid to produce 2.01
grams of water, what is the percent yield? (55.8%)
______________
10. Lime, CaO, reacts with hydrochloric acid to form calcium chloride and
water. How many moles of HCl would be required to react with 7.5 moles of
lime? How many moles of water would be formed? (15 mol HCl; 7.5 mol water)
______________
For each of the following write balanced chemical equations and then solve the
problem.
11. What is the maximum number of grams of PH3 that can be formed when
6.2 g of phosphorus reacts with 6.0 g of hydrogen to form PH3?
______________
12. Copper is formed when aluminum reacts with cupric sulfate in a singlereplacement reaction. How many grams of copper can be obtained when 29.0 g
of Al reacts with 156 g or cupric sulfate?
______________
13. If you begin with 1250 g of N2 and 225 of H2 in the reaction that forms
ammonia gas (NH3), how much ammonia will be formed? What is the limiting
reagent? How much of the reagent is left when the maximum amount of
ammonia is formed?
______________
AP Chem Summer Assignment Worksheet #7
Predicting Reaction Products
Balance the equations and predict the products and states of matter (assumer reactions
are taking place at STP) for the following reactions. If no reaction occurs write ‘NR’.
1)
____ Na + ____ FeBr3 
2)
____ NaOH + ____ H2SO4 
3)
____ C2H4O2 + ____ O2 
4)
____ NH3 + ____ H2O 
5)
____ PbSO4 + ____ AgNO3 
6)
____ PBr3 
7)
____ HBr + ____ Fe 
8)
____ KMnO4 + ____ ZnCl2 
9)
____MnO2 + ____ Sn(OH)4 
10)
____ O2 + ____ C5H12O2 
11)
____ H2O2 
12)
____ PtCl4 + ____ Cl2 