Electrons and Periodicity Test Rev

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Electrons and Periodicity Test Review
Word Bank 1-10
Atomic number
18
3
Ground state
8
Group number
Increases
Excited
Neon
6
1. A neutral atom of argon contains (how many?)
lo
electrons.
2. When all of the electrons in an atom are in the lowest available energy levels, the atom is in
the n^nimc^ S-VCL-i€.
3. A neutral atom containing ten negative charges is the element
4. As an electron's distance from the nucleus increases, its energy content
'
5. The position of an atom in the periodic table and the number of its electrons are both given by
its <g.-fcnfn\f
6. The maximum number of valence electrons possible in any outermost shell is
7. The number of valence electrons increases with increase in OIVDULp Al jUT\t>£/(~
from the beginning to the end of period 2.
8. If an electron has absorbed energy and has shifted to a higher energy level, the electron is
said to be a \fr\-\ff\ _
.
9. In any p sublevel, there are how many p orbitals
/j _
.
10. The maximum number of electrons possible in any p sublevel is
Word Bank 11 -20
More
Nucleus
P sublevel
2
S sublevel
2
8
Germanium
Krypton
10
Farther
Calcium
4
Stable
1 1 .A 3d orbital has fTXPf^
energy than a 3p orbital.
12. The only two kinds of orbitals which may occur in the outermost shell are the
g*ibu;.M£A
&
13. The number of valence electrons in Helium is 9> , but the number of valence electrons in all
other inert gases is *PS
14. The element having atomic number 36 is
V^fVI ofo IA_
. The number of electrons
in its 3d sublevel is _ |t3_
.
15. The electron configuration 1s22s22p63s23p64sLis that of element C/llfJLdrCi
.
16. The electron configuration 1s22s22p63s23p64s23d104p/t-is that of the element (qp/lYVl{VtU.fV\
which contains (how many?) _
£f_
electrons in its outermost shell?
17. An atom is chemically
S"\Q-fo^€__
when all of the orbitals in the
outermost shell are completely filled.
18. Bohr postulated that electrons could only exist in certain paths around the fXilfifflA
19. No more than
- A_
electrons can be accommodated in an orbital.
20. According to Bohr, the more energy the electron possesses, the •tQL<"-H\€/" it is from the
nucleus
Multiple choice
21. Spectral lines (light) of the elements are caused by
(a) electrons falling to lower energy levels
c. electrons jumping to higher energy levels
b. electrons turning in their orbital paths
d. the sympathetic vibration of the nucleus
22. The outermost shell of any atom can hold a maximum of
(a) 8 electrons
b. 2 electrons
c. 18 electrons
d. 32 electrons
23. The number of sublevels in the fifth energy level is
a. 7
b. 3
c. 5
©4 S o ^ j f
24. The 4f sublevel is filled next after
a. the 6s sublevel
b. the 5p sublevel (o)the 5s. level
d. the 4d sublevel
25. The maximum number of electrons in the fourth principal energy level is
a. 8
b. 16
(©32
d. 64
26. A p orbital is
a. best described as a cube b. sphere shaped
27. The sublevel of lowest energy is
a. 3d
b. 3p
(c*)2s
28. 1s2 is the representation of
a. H
b. F
c. Hg
c. too complicated to describe (dijfieanut
d. 2p
(d^He
Base your answers to questions 29-33 on the following electron configuration of a
neutral atom:
1s22s22p63s23p4
29. What is the number of valence electrons in this atom?
\Q
30. The total number of electrons in the second energy level of this atom is
. *•
'
31 . How many unpaired electrons are in an atom of this element in the ground
state?
>
_
32. What is the total number of electron energy levels in this atom?
.'j
33. What element is this atom?
Provide STANDARD, NOBLE GAS CONFIGURATION, AND DOT STRUCTURE for the following
Copper StandardShort
Dot Structure
Aluminum Standard-
\S ZS 2.^)
33
Short hand-
_
* >
Dot Structure
Barium Standard- \^ 2s^ 2^ 5s*3p"
'°
Short handDot Structure
Determine if the following electron configurations are valid. If not, explain why:
1 . 1 s22s22p63s23p64s24d1V r\h4 ygJJA , £tlV ^'"o^W-r 4s2"
2. 1s22s22p63s33d5 r\tA MoUA^iU 5p filter .%, AiNOD onK
onKf ??.e.
3. {Raj 7s2S? 'ZaA\usK mnnD-V Vv
4. [Kri 5s24d1°5p5
ci .
ho
5. [Xel
Which rule is being violated in the following orbital notation diagrams? Explain why.
Periodic Trends
1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen,
potassium
5t><\<x\X&5-T
^
toAQes-f
*J
C_) (_, . rr V
>
rS
loyJ€5r —
2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum
3. Which is larger, Ca2* or Ca and why? CQ_ Gx r\j£, Los\ Q, c4. How does the ionic.radius of a nonmetal compare with its atomic radius?
5. Define ionization ejiergy.
-Vo
- -from
6. Define electronegati
otoiU-Vvf-Vo o.Woc\ e- -Vts OJT\
7. Rank each of the following in order of INCREASING ionization energy
O, S, Ge
C, Pb, F
Be, Ba, B
8. Rank each of the following in order of DECREASING electronegativity
As, Se, Sn
I, Ru, Hf
Sb, N, Be,
Light and Waves
1 . Calculate the energy (E) and wavelength (X) of a photon of light with a frequency of
6.165 x10 14 Hz. E-A./
- 7- 8?£
2. Calculate the frequency of light that has a wavelength of 4.25 x 1 0"9m. Identify the type of
electromagnetic radiation, (use the EM spectrum on back of this page)
MM
3. Find the energy of microwave radiation with a frequency of 7.91 x 1010 Hz
34 A ruby laser produces red light that has a wavelength of 600 nm. Calculate its energy in joules.
Label the wave: Crest, Trough, Origin, Amplitude, and Wavelength
'cres-V
Use the picture at the bottom of the page
1. Rank the types of waves from longest to shortest wavelength:
J
M't&iHf./lA.X/, y\f\
2. Which color has the most energy? N/lfiufL-f
3. Which color has the least energy?
4. On the EM Spectrum, which type of wave has the most energy?
5. On the EM Spectrum, which type of wave has the least energy?
6. On the EM Spectrum, which type of wave has the highest frequency?
7. On the EM Spectrum, which type of wave has the lowest frequency? r\Q/J (
8. Yellow light has a longer wavelength than green light. Which color of light has the higher
frequency? faf££f\
9. Green light has a lower frequency than blue light. Which color of light has a longer
wavelength?
^)T-gfT\
10. The higher the frequency, the
10*Hz
KAtyTVCr
11 .The longer the wavelength, the
1.0\NlgjT
12.The longer the wavelenqth, the
IDNNldA
104Hz
10*Hz
10*Hz
!0'§Hz
(higher/lower) the energy.
(higher/lower) the energy.
(higher/lower) the frequency.
101lHz
mm
Visible tight
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G
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