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Midterm 2015
Regents
Chemistry
Part A
January 29, 2015
8:00 am
Ms. Spaman
Mr. Meredith
Mr. Schlesing
Regents Chemistry
Midterm Test
Part A
1 - 50 Multiple Choice
1. Which substance can be decomposed by a chemical
change?
1) calcium
3) copper
2) potassium
4) water
2. At STP, which substance has particles arranged in a
regular geometric pattern, also known as a
crystalline lattice structure?
1) Ne
3) Hg
2) Zn
4) He
3. What occurs when a substance melts?
1) It changes from solid to liquid, and heat is
absorbed.
2) It changes from solid to liquid, and heat is
released.
3) It changes from liquid to solid, and heat is
absorbed.
4) It changes from liquid to solid, and heat is
released.
5. Which statement is an identifying characteristic of
a mixture?
1) A mixture can consist of a single element.
2) A mixture can be separated by physical means.
3) A mixture must have a definite composition by
weight.
4) A mixture must be homogeneous.
6. Which atom in the ground state has a partially
filled second electron shell?
1) hydrogen atom
3) potassium atom
2) lithium atom
4) sodium atom
7. Compared to the charge and mass of a proton, an
electron has
1) the same charge and a smaller mass
2) the same charge and the same mass
3) an opposite charge and a smaller mass
4) an opposite charge and the same mass
8. An atom in the excited state can have an electron
configuration of
1) 2 - 8 - 2 (ls22s22p63s2)
2) 2 - 7 - 2 (ls12s22p53s2)
3) 2 - 8 - 1 (ls22s22p63s1)
4) 2 - 7 (ls22s22p5)
4. Given the key:
Which particle diagram represents a sample
containing the compound CO(g)?
9. What is the total number of protons and neutrons in
the nuclide 80
35Br?
1) 35
3) 80
2) 45
4) 115
10. Which electron-dot symbol represents an atom of
chlorine in the ground state?
1)
3)
1)
2)
2)
4)
Page 1
3)
4)
Regents Chemistry
Midterm Test
Part A
1 - 50 Multiple Choice
11. An experiment in which alpha particles were used
to bombard thin sheets of gold foil led to the
conclusion that an atom is composed mostly of
1) empty space and has a small, negatively
charged nucleus
2) empty space and has a small, positively
charged nucleus
3) a large, dense, positively charged nucleus
4) a large, dense, negatively charged nucleus
12. Which Group 16 element undergoes natural
radioactive disintegration?
1) Po
3) Se
2) S
4) Te
13. At STP, both diamond and graphite are solids
composed of carbon atoms. These solids have
1) the same crystal structure and the same
properties
2) the same crystal structure and different
properties
3) different crystal structures and the same
properties
4) different crystal structures and different
properties
14. Given the balanced particle-diagram equation:
Which statement describes the type of change and the chemical properties of the product and reactants?
1) The equation represents a physical change, with the product and reactants having different chemical properties.
2) The equation represents a physical change, with the product and reactants having identical chemical properties.
3) The equation represents a chemical change, with the product and reactants having different chemical properties.
4) The equation represents a chemical change, with the product and reactants having identical chemical properties.
15. Given the following ground state electron
configuration, 2 - 8 - 18 - 6
(or ls22s22p63s23p63d104s24p4) What is the total
number of electrons in the principal energy level
that has the greatest amount of energy?
1) 4
3) 18
2) 8
4) 6
16. Which atom in the ground state requires the least
amount of energy to remove its valence electron?
1) lithium atom
3) rubidium atom
2) potassium atom
4) sodium atom
Page 2
Regents Chemistry
Midterm Test
17. An element that is malleable and a good conductor
of heat and electricity could have an atomic
number of
1) 16
3) 29
2) 18
4) 35
18. The transfer of electrons from sodium atoms to
chlorine atoms results in the formation of
1) metallic bonds
3) nonpolar bonds
2) polar covalent bonds 4) ionic bonds
19. The atomic mass unit (amu) is defined as exactly
1/12 the mass of an atom of
1) 12
3) 24
6 C
12Mg
14
2) 6 C
4) 26
12Mg
20. The bonds in all network solids are
1) covalent
3) metallic
2) ionic
4) nonpolar
21. Which element has a crystalline lattice composed
of positive ions through which electrons flow
freely?
1) bromine
3) carbon
2) calcium
4) sulfur
22. What is the chemical formula for copper (II)
chlorate?
1) Cu2Cl
3) Cu2ClO3
2) CuCl2
4) Cu(ClO3)2
Part A
1 - 50 Multiple Choice
25. Given the reaction:
H2 + Cl2 →2HCl
Which statement best describes the energy change
as bonds are formed and broken in this reaction?
1) The breaking of the Cl–Cl bond releases energy.
2) The breaking of the H–H bond releases energy.
3) The forming of the H–Cl bond absorbs energy.
4) The forming of the H–Cl bond releases energy.
26. Which is an empirical formula?
1) C2H2
3) H2O2
2) H2O
4) C6Hl2O6
27. Which symbol represents an atom in the ground
state with the most stable valence electron
configuration?
1) B
3) Li
2) O
4) Ne
28. Which type of bond is formed between the carbon
and oxygen atoms in a CO2 molecule?
1) nonpolar covalent
3) ionic
2) polar covalent
4) metallic
29. Which electron-dot structure represents a non-polar
molecule?
23. How does the size of an aluminum atom change
when it becomes an ion with a charge of 3+?
1) It becomes smaller by losing 3 electrons.
2) It becomes smaller by gaining 3 electrons.
3) It becomes larger by losing 3 electrons.
4) It becomes larger by gaining 3 electrons.
1)
24. In the electron cloud model of the atom, an orbital
is defined as the most probable
1) charge of an electron
2) conductivity of an electron
3) location of an electron
4) mass of an electron
2)
3)
4)
30. Which element has an atom with the greatest
attraction for electrons in a chemical bond?
1) As
3) N
2) Bi
4) P
31. Which element is a nonmetallic liquid at room
temperature?
1) hydrogen
3) mercury
2) oxygen
4) bromine
Page 3
Regents Chemistry
Midterm Test
Part A
1 - 50 Multiple Choice
32. The properties of elements are periodic functions
of their
1) mass numbers
3) atomic radii
2) atomic masses
4) atomic numbers
38. Atoms of different isotopes of the same element
differ in their total number of
1) electrons
3) protons
2) neutrons
4) valence electrons
33. The elements in Period 3 all contain the same
number of
1) protons
2) neutrons
3) valence electrons
4) occupied principal energy levels
39. As the elements in Group 15 are considered in
order of increasing atomic number, which sequence
in properties occurs?
1) nonmetal → metalloid → metal
2) metalloid → metal → nonmetal
3) metal → metalloid → nonmetal
4) metal → nonmetal → metalloid
34. Which is an example of a metalloid?
1) sodium
3) silicon
2) strontium
4) sulfur
35. Which atom forms an ion with the largest radius?
1) I
3) Cl
2) Br
4) F
36. The diagram below represents the nucleus of an
atom.
40. Which element in Period 2 of the Periodic Table is
the most reactive nonmetal?
1) carbon
3) oxygen
2) nitrogen
4) fluorine
41. Which element in Period 3 exists as diatomic
molecules at STP?
1) argon
3) aluminum
2) chlorine
4) sodium
42. Which sample of water contains particles having
the highest average kinetic energy?
1) 25 mL of water at 95°C
2) 45 mL of water at 75°C
3) 75 mL of water at 75°C
4) 95 mL of water at 25°C
What are the atomic number and mass number of
this atom?
1) The atomic number is 9 and the mass number is
19.
2) The atomic number is 9 and the mass number is
20.
3) The atomic number is 11 and the mass number
is 19.
4) The atomic number is 11 and the mass number
is 20.
37. Which element is in Group 2 and Period 7 of the
Periodic Table?
1) magnesium
3) radium
2) manganese
4) radon
43. Which aqueous solution is colored?
1) CuSO4(aq)
3) KCl(aq)
2) BaCl(aq)
4) MgSO4(aq)
44. Which element can be brittle or soft in the solid
phase and is a poor conductor of heat and
electricity?
1) calcium
3) strontium
2) sulfur
4) copper
45. Magnesium and calcium have similar chemical
properties because a magnesium atom and a
calcium atom have the same
1) atomic number
2) mass number
3) total number of electron shells
4) total number of valence electrons
Page 4
Regents Chemistry
Midterm Test
46. Which element is an alkali metal?
1) Na
3) Al
2) Mg
4) Cl
Part A
1 - 50 Multiple Choice
49. Which mass measurement contains a total of three
significant figures?
1) 22.0 g
3) 220 g
2) 22.00 g
4) 2200 g
47. Given:
(52.6 cm) × (1.214 cm)
50. Which laboratory glassware is shown in the
diagram below?
What is the product expressed to the correct
number of significant figures?
1) 64 cm2
3) 63.86 cm2
2
2) 63.9 cm
4) 63.8564 cm2
48. The diagram below shows a portion of a graduated
cylinder.
1) Beaker
2) Erlenmeyer Flask
What is the meniscus reading in milliliters?
1) 17.60
3) 17.80
2) 17.70
4) 18.40
Page 5
3) Graduated Cylinder
4) Watch Glass
Regents
Chemistry
Midterm
Part B and Part C
Regents Chemistry
Midterm Test
Mr. Schlesing
Part B
51 - 75 Multiple Choice
51. How many kilojoules are equivalent to 10 joules?
1) 0.001 kJ
3) 1000 kJ
2) 0.01 kJ
4) 10,000 kJ
58. The normal boiling point of water is equal to
1) 173 K
3) 373 K
2) 273 K
4) 473 K
52. What is the total number of Joules of heat that must
be absorbed to change the temperature of 100.
grams of H2O from 25.0ºC to 30.0ºC?
1) 420.
3) 10500
2) 2100
4) 13000
59. The graph below represents changes of state for an
unknown substance.
53. What is the total number of joules released when a
5.00-gram sample of water changes from liquid to
solid at 0°C?
1) 334 J
3) 2260 J
2) 1670 J
4) 11 300 J
54. Solid A at 80ºC is immersed in liquid B at 60ºC.
Which statement correctly describes the energy
changes between A and B?
1) A releases heat and B absorbs heat.
2) A absorbs heat and B releases heat.
3) Both A and B absorb heat.
4) Both A and B release heat.
55. Which phase change is exothermic?
1) H2O(s) → H2O(…)
3) H2O(s) → H2O(g)
2) H2O(…) → H2O(s)
4) H2O(…) → H2O(g)
56. Which Kelvin temperature is equal to –73ºC?
1) 100 K
3) 200 K
2) 173 K
4) 346 K
57. A student investigated the physical and chemical
properties of a sample of an unknown gas and then
identified the gas. Which statement represents a
conclusion rather than an experimental observation?
1) The gas is colorless.
2) The gas is carbon dioxide.
3) When the gas is bubbled into limewater, the
liquid becomes cloudy.
4) When placed in the gas, a flaming splint stops
burning.
What is the boiling temperature of the substance?
1) 0ºC
3) 70ºC
2) 20ºC
4) 40ºC
60. Which equation is correctly balanced?
1) CaO + 2H2O → Ca(OH)2
2) NH3 + 2O2 → HNO3 + H2O
3) Ca(OH)2 + 2H3PO4 → Ca3(PO4)2 + 3H2O
4) Cu + H2SO4 → CuSO4 + H2O + SO2
61. Given the balanced equation representing a
reaction:
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)
Which type of reaction is represented by this
equation?
1) decomposition
3) single replacement
2) double replacement 4) synthesis
Page 7
Regents Chemistry
Midterm Test
Part B
51 - 75 Multiple Choice
Mr. Schlesing
62. The graph below represents the uniform heating of
a substance, starting with the substance as a solid
below its melting point.
Which line segment represents an increase in
potential energy and no change in average kinetic
energy?
1) AB
3) CD
2) BC
4) EF
63. Given the unbalanced equation:
NaOH + H3PO4 → Na3PO4 + H2O
When the equation is correctly balanced, the
coefficient of H2O will be
1) 1
3) 3
2) 2
4) 4
64. What is the gram formula mass of
Mg(ClO3)2?
1) 107 g
3) 174 g
2) 142 g
4) 191 g
66. The percent by mass of carbon in HC2H3O2 is
equal to
1)
3)
2)
4)
67. What is the mass of 2.0 moles of NO2?
1) 92 grams
3) 46 grams
2) 60. grams
4) 30. grams
68. In the formula X2(SO4)3, the X represents a metal.
This metal could be located on the Periodic Table in
1) Group1
3) Group 13
2) Group 2
4) Group 14
69. Which species represents a chemical compound?
1) N2
3) Na
2) NH4+
4) NaHCO3
70. A real gas would behave most like an ideal gas
under conditions of
1) low pressure and low temperature
2) low pressure and high temperature
3) high pressure and low temperature
4) high pressure and high temperature
65. What is the total number of atoms of oxygen in the
formula Al(ClO3)3 • 6H2O?
1) 6
3) 10
2) 9
4) 15
Page 8
Regents Chemistry
Midterm Test
Mr. Schlesing
71. Which graph represents the relationship between
pressure and volume for a sample of an ideal gas at
constant temperature?
1)
Part B
51 - 75 Multiple Choice
72. Based on Reference Table H, which substance has
the weakest intermolecular forces?
1) ethanoic acid
3) propanone
2) ethanol
4) water
73. According to Reference Table H, what is the
boiling point of ethanoic acid at 80 kPa?
1) 28°C
3) 111°C
2) 100°C
4) 125°C
2)
3)
74. A sample of a gas has a volume of 40. milliliters at
76.0 kPA. What will be the new volume of the gas
if the pressure is increased to 80.0 kPa, temperature
remaining constant?
1) 80 ml
3) 38 ml
2) 42 ml
4) 20 ml
75. A rigid cylinder with a movable piston contains a
2.0-liter sample of neon gas at STP. What is the
volume of this sample when its temperature is
increased to 30.°C while its pressure is decreased
to 90. kilopascals?
1) 2.5 L
3) 1.6 L
2) 2.0 L
4) 0.22 L
4)
Page 9
Part B
-
– Constructed Response Questions [5 pts total]
Place all answers on the answer sheet
Base your answers to questions 76 and 77 on the table below.
Naturally Occurring Isotopes of Copper
Isotope Notation
Percent Natural
Atomic Mass
Abundance (%)
(atomic mass units, u)
Cu–63
69.17
62.930
Cu–65
30.83
64.928
76. What is the total number of neutrons in Cu–65? [1pt]
77. Show a correct numerical setup for calculating the atomic mass of copper. [1pt]
Base your answers to questions 78 and 79 on the information below.
A glass tube is filled with hydrogen gas at low pressure. An electric current is passed through the gas,
causing it to emit light. This light is passed through a prism to separate the light into the bright, colored lines of
hydrogen’s visible spectrum. Each colored line corresponds to a particular wavelength of light. One of
hydrogen’s spectral lines is red light with a wavelength of 656 nanometers.
Tubes filled with other gases produce different bright-line spectra that are characteristic of each kind of
gas. These spectra have been observed and recorded.
78. Explain, in terms of electron energy states and energy changes, how hydrogen’s bright-line spectrum is
produced. [1pt]
79. A student measured the wavelength of hydrogen’s visible red spectral line to be 647 nanometers. Show
a correct, numerical setup for calculating the student’s percent error. [1pt]
Base your answers to question 80 on the table below.
Compound
H2O
H2S
H2Se
H2Te
Boiling Point
100. °C
-60.7 °C
-41.5 °C
-2.2 °C
80. Explain, in terms of intermolecular forces, why water has a higher boiling point than H2S, H2Se, and
H2Te. [1pt]
Part C
– Constructed Response Questions [20 pts total]
Midterm Exam
Directions: Choose 4 of the 6 groups in this part of the examination. For the 4 groups that you choose to
answer, make sure you answer all the questions within those groups. If you complete all 6 groups on your
answer sheet, only the first 4 will be graded. Make sure that you answer the questions for each group in the
correct location on the answer sheet. (20 points)
Group 1)
a) Given the information about the elements in the table below, fill in the missing information on
the corresponding table on your answer sheet. [1pt]
# of Protons Electron configuration Element Symbol
of atom
12
2–8–2
11
Na
2–8
Ne
8
2–5
B
***Use only the elements from the above table (a) to answer questions b), c), d), & e)
b) The element with the highest first ionization energy? [1pt]
c) The element that will form a negative ion in a compound? [1pt]
d) The element with the greatest number of unpaired electrons in its Lewis dot (electron dot)
diagram? [1pt]
e) The metal that would combine with oxygen in a one-to-one ion ratio? [1pt]
Group 2)
Answer the following questions (a,b,c,d) about a compound that is created by the elements of
calcium and fluorine.
a)
c)
d)
Describe the type of chemical bond that would occur in a compound that consists of calcium
and fluorine atoms. [1pt]
Describe a specific chemical or physical property for a solid of this compound (Your
property can’t be that it is a solid, that information is given in the problem.) [1pt]
Give the correct chemical name for this compound of calcium and fluorine. [1pt]
Draw the Lewis Structural Formula (Dot Diagrams) for this compound. [1pt]
e)
Write the correct name of Ni(NO3)2. [1pt]
b)
Group 3)
For each of the following, give the symbol of the element described.
a)
b)
c)
d)
e)
an alkaline earth metal found in Period 4. [1pt]
the element in Period 4 with the greatest attraction for an electron in a chemical bond. [1pt]
the most metallic element found in Group 15. [1pt]
a diatomic molecule that is stable due to a triple covalent bond in its molecule. [1pt]
a diatomic molecule that is a liquid at room temperature. [1pt]
Group 4)
A student wished to perform a lab to calculate the percent composition by mass of water in a
hydrated crystal. The student first obtained the mass of an empty, dry evaporating dish. The
student then placed a small amount of the hydrated crystal in the evaporating dish and weighed it.
The student’s data is shown below:
Mass of empty evaporating
11.70 g
dish
Mass of evaporating dish +
14.90 g
hydrated crystal
a) Explain at least 2 additional lab procedures that this student will need to do in order to gather enough
data to calculate the percentage of water in this hydrated crystal. [2pts]
b) At the end of this lab, the student found the mass of the anhydrous crystal (dehydrated crystal) to be
2.83 grams. Calculate using significant figures, the mass of the water found in the hydrated crystal.
(show your work on the answer sheet) [2pts]
c) Calculate the percentage of water in the original hydrated crystal. (show your work on the answer
sheet) [1pt]
Group 5) The electron configuration for the phosphorus atom is 2–8–5 or 1s22s22p63s23p3. Indicate for this
atom:
a)
b)
c)
d)
e)
the number of completely filled principal energy levels. [1pt]
the type of bond that forms when its chemically combines with chlorine. [1pt]
the number of protons in its nucleus. [1pt]
the electron dot diagram (Lewis dot diagram) for an atom of this element. [1pt]
the specific ion it will most likely form when bonding with a metal atom. [1pt]
Group 6) Many periodic trends can be observed on the modern periodic table. Answer the following questions
about periodic trends on your answer sheet.
a) Graph the periodic trend in atomic radius for Period 3 on the appropriate graph on your answer
sheet. [1pt]
b) Explain the cause for the observed periodic trend in atomic radius for Period 3 elements. [1pt]
c) Graph the group trend in atomic radius for Group 2 on the appropriate graph on your answer sheet.
[1pt]
d) Explain the cause for the observed group trend in atomic radius for Group 2 elements.
e) Ions of Group 2 elements are found to have radii smaller than that of the individual atoms, explain
the cause of this observed trend. [1pt]

End of Exam
Part A = ______
Name: ______________________________
Teacher: _________________
Class: ____________ Regents Chemistry Midterm Answer Sheet
Total Score
Part B = ______
Part C = ______
Part A – do all 50 questions.
1. _____
11. _____
21. _____
31. _____
41. _____
2. _____
12. _____
22. _____
32. _____
42. _____
3. _____
13. _____
23. _____
33. _____
43. _____
4. _____
14. _____
24. _____
34. _____
44. _____
5. _____
15. _____
25. _____
35. _____
45. _____
6. _____
16. _____
26. _____
36. _____
46. _____
7. _____
17. _____
27. _____
37. _____
47. _____
8. _____
18. _____
28. _____
38. _____
48. _____
9. _____
19. _____
29. _____
39. _____
49. _____
10. _____
20. _____
30. _____
40. _____
50. _____
Part A Score =
Part B – do all questions.
51. _____
56. _____
61. _____
66. _____
71. _____
52. _____
57. _____
62. _____
67. _____
72. _____
53. _____
58. _____
63. _____
68. _____
73. _____
54. _____
59. _____
64. _____
69. _____
74. _____
55. _____
60. _____
65. _____
70. _____
75. _____
76. ___________
77.
78.
_________________________________________________________________________________
______________________________________________________
______________________________________________________
79.
80.
________________________________________________________________________________
______________________________________________________
______________________________________________________
Part B Score =
Part C - complete 4 of the 6 groups only!
Group 1
a)
# of Protons
12
11
Electron configuration
of atom
2–8–2
Element Symbol
[1pt]
Na
Ne
2–8
8
2–5
B
b) _______________________________ [1pt]
c) _______________________________ [1pt]
d) _______________________________ [1pt]
e) _______________________________ [1pt]
Group 2
a) ____________________________________________________________________
__________________________________________________________________[1pt]
b) ___________________________________________________________________
___________________________________________________________________[1pt]
c) __________________________________ [1pt]
d)
[1pt]
e) ___________________________________ [1pt]
Total Points on this Page =_______
Part C – Continued
Group 3
a) _____________ [1pt]
b) _____________ [1pt]
c) _____________ [1pt]
d) _____________ [1pt]
e) _____________ [1pt]
Group 4
a) #1 Step______________________________________________________________
______________________________________________________________________
#2 Step______________________________________________________________
_________________________________________________________________[2pts]
b) Show work in the box below and circle your final answer. [2pts]
c) Show work in the box below and circle your final answer. [1pt]
Group 5
a) ________________ [1pt]
b) ________________ [1pt]
c) ________________ [1pt]
d) ________________ [1pt]
e) ________________ [1pt]
Total Points on this Page = ______
Group 6 a.)
Atomic Radii of Period 3
b.) ______________________________________
190
__________________________________________
180
170
160
__________________________________________
Atomic Radius (picometers)
150
140
__________________________________________
130
120
__________________________________________
110
100
__________________________________________
90
80
70
60
50
40
30
20
10
0
Na
Mg
Al
Si
P
S
Cl
Ar
Period 3 Elements
c.)
Atomic Radii of Group 2
d.) _________________________________________
240
__________________________________________
230
220
210
__________________________________________
200
Atomic Radius (picometers)
190
__________________________________________
180
170
__________________________________________
160
150
__________________________________________
140
130
120
110
100
90
80
70
0
Be
Mg
Ca
Sr
Ba
Ra
Group 2 elements
e.) ______________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
Total Points on this Page = _________
k>3
Name:
ftn,.
Teacher:
*t
V1
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Part B Score =
Paft
C
Group
- do 4 of the 6 groups only!
I
a)
# of Protons
Electron configuration
of atom
2-8-2
t2
l1
7-8-
(a
7
Na
Ne
o
2-5
t$
2-3
N.-
[1pt]
lY\9.
(
2-8
'la
8
b)
Element Symbol
B
[1pt]
c) C- .* N
trou
[1pt]
M^-
uy
Group
2
lrpq
a)
lptl
G^,2
< - (;,!
b)
€^
c)
d)
Co\ci.,n^,
ft.r.ci
d.--
d-J"Lrl;'dNick
\
trptl
[1pt]
[1pt]
Total Points on this Page =
- Continued
C=-?
Group 3
Paft
C
"l
ol B.
[1pt]
[1pt]
c)
[1pt]
l"L
d)
"y
Group 4
6cr-
grptl
ll'o
dI'-L {.
a) #1 Step__:
.4-q.\ -L/
#2 Step
b)
[1pt]
.fr(
q-,L=
2ptsl
Show work in the box below and circle your final answer. [2pts]
hy"l*F,, * cn:dLL nr"== rK itL
y
[ (,7ot b",U\L
11 72
c-r
.%feo
((r
nswer. [1pt]
Show work in the box
% Lro';ffi-,.n,o<>
.3?>
"/ #ru=6'o.ao
oc 0-(
+T
Group 5
a)
[1pt]
b) (
c)
d)
e)
.?'
P-t^
_ tlptl
[tpt]
Total Points on this Page:
Group 6 a.)
c.)
Atomic Radii of Period
ul -{h-
3
A,,^
fl6r.r,>- Q,&i->
Atomic Radii of Group 2
Group 2 elements
';
A'=-
d."-
f
er."t*
u (*(
Total Points on this Page
=