Name: __________________________________________
Chemistry -Unit 3 Periodic Test Review
The periodic table and its trends
1) On the table to the right label the location for these groups
– Halogens, Noble Gases, Alkaline Earth Metals, Alkali Metals,
and Transition Metals
2) On the periodic table below circle the most electronegative
element and put a square around the least electronegative
element.
3) Shade the element with the highest ionization energy red
and the element with the lowest blue.
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5) On the table above - number the periods.
6) Shade period 4 in blue.
7) The rows are periods and the columns are _________.
8) The periodic table is organized according to increasing
__________ ___________
9) On the table to the left – use arrows to show the trend of
increasing atomic size & radius. Circle the atom with the largest
atomic size & radius.
10) Shade the metals in red, the nonmetals in blue, and metalloids
in green.
Identify the group by its’ description (halogens, alkali earth
____________________ 11) Have 1 valence electron
____________________ 12) Have 8 valence electrons
____________________ 13) Have 7 valence electrons
____________________ 14) Have 2 valence electrons
____________________ 15) The least reactive elements
metals, noble gases, transition metals, and alkali metals)
____________________ 16) The most reactive nonmetals
____________________ 17) The most reactive metals
____________________ 18) Reacts explosively with
oxygen and water
____________________ 19) Used to make coins &jewelry.
Match to its correct definition (electronegativty and ionization energy)
____________________ 20) Energy required to remove an electron from an atom
____________________ 21) The ability of atom to attract electrons.
22) List 3 other elements that will have similar chemical properties to Nitrogen. Why do they have similar properties?
23) How many electrons does an atom of Oxygen have? _____ How many electrons does 0-2 have? _____
24) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why fluorine
holds on to its electrons so well)
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Electron configuration
Refer to the configuration to answer the following 4 questions: 1s2 2s2 2p6 3s2 3p6 4s2
25) Which element is this for? ____________________
27) In which group #? _______
26) In which period is this element found in?______
27) How many electrons are in the 3rd energy level? ____
28) Re-write the electron configuration of this element if it became an ion with a +2 charge.
29) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found.
30) How many orbitals are in each sublevel? a. S = ___
b. P = ___
c. D = ___
d. F = ____
31) How many electrons can fit into 1 orbital? _____
32) Is the following electron configuration sketch correct? Explain.
3s
3p
4s
3d
33) On the table to the left – color and label these blocks:
 the s block (red)
 the d block (green)
 the p block (yellow)
 the f block (brown)
34) Identify the blocks where these groups are found –
a. Halogens = ____ block
b. Alkaline Earth Metals = _____ block
c. Alkali Metals = ______ block
d. Rare Earth Metals = ______ block
e. The Noble Gases = _____ block
f. The Transition Metals = _______ block
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Photons and the Electromagnetic Spectrum
35) Use the known spectrum samples at the
right to identify the unknowns below.
36) An electron that is closest to the
nucleus possible (at the lowest energy level
possible) is said to be in its ___________
_________________.
37) When an electron jumps up to a higher
energy level and then falls back to its
ground state a ___________ is released.
38) Please circle the answer that correctly
completes the sentence.
The amount of energy released by an
electron jumping from the 4th energy level
back to its ground state at the 3rd energy level will
always release a photon with a different or
variable/specific or quantized amount of energy.
39) The color spectra (types of colors produced) of
a star can be used to identify the types of
______________ present in the star or chemical
sample.
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