Chemistry –Periodic Table 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 table below – use arrows to show the trends of
increasing electronegativity and ionization energy. Use horizontal
and vertical arrows.
3) Also, circle the most electronegative element and put a square
around the least electronegative element.
4) Shade the element with the highest ionization energy red and
the element with the lowest blue.
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
__________ ___________ (the #’s in the boxes)
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9) On the table to the left – use arrows to show the
trend of atomic size (radius). Point arrows from
smallest radii to largest. Use a horizontal arrow and a
vertical arrow.
10) Shade the metals in red, the nonmetals in blue, and
metalloids in green.
Match the group to the correct description (halogens, alkali earth metals, noble gases, transition metals, and alkali
metals)
____________________ 11) Have 1 valence electron
____________________ 12) Have 8 valence electrons
____________________ 12) Have 7 valence electrons
____________________ 13) Have 2 valence electrons
____________________14) The least reactive elements
____________________ 15) The most reactive nonmetals (gases at room temperature)
____________________ 16) The most reactive metals
____________________ 17) Reacts readily with oxygen and water
____________________ 18) Used to make coins and jewelry.
Match to its correct definition (electronegativty and ionization energy)
____________________ 19) Energy required to remove an electron from an atom
____________________ 20) The ability of atom to attract electrons.
21) List 3 other elements that will have similar chemical properties to Nitrogen and explain why.
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22. Circle the element in the pair has the larger ionization energy. Explain why.
a. Li, N
b. Kr, Ne
c. Cs, Li
23. Explain the octet rule. _____________________________________________________
______________________________________________________________________
24. Circle the element in the pair is more electronegative. Explain Why?
a. K, As
b. N, Sb
c. Sr, Be
25. Periodic law states that elements show a
a. repetition of their physical properties when arranged by increasing atomic radius.
b. repetition of their chemical properties when arranged by increasing atomic radius.
c. periodic repetition of their properties when arranged by increasing atomic number.
d. periodic repetition of their properties when arranged by increasing atomic mass.
26. Elements in the same group of the periodic table have the same:
a. number of valence electrons
b. physical properties
c. number of electrons
27. Which of the following is NOT true of an atom, other than Helium, obeying the octet rule?
a. obtains a full set of 8 valence electrons
b. acquires the valence electrons of a noble gas
c. possess 8 electrons in total
d. has a s2p6 valence configuration
28. Moving down the periodic table, which two atomic properties follow the same trend?
a. atomic radius, ionization energy
b. atomic radius, electronegativity
c. ionization energy, electronegativity
d. none of the above
29. Which will form a larger ionic radii than its’ parent atom?
a. cation
Explain your choice!
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(+ ion)
b. anion (- ion)
30) How many electrons does an atom of Oxygen have? _____ How many electrons does 0-2 have? _____
31) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why
fluorine holds on to its electrons so well)
Electron configuration
Refer to the configuration to answer the following 4 questions –
1s2 2s2 2p6 3s2 3p6 4s2 3d6
32) Which element is this for? ____________________33) In which period is this element found in?______
In which group #? _______
34) How many electrons are in this elements 3rd energy level? _____
35) Re-write the electron configuration of this element if it became an ion with a +2 charge.
36) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found.
37) How many orbitals are in each sublevel? a. S = ___
b. P = ___
38) How many electrons can fit into 1 orbital? _____
39) What do the quantum numbers tell us about an atomic orbital?
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c. D = ___
d. F = ____
40) Is the following orbital notation for the 3rd and 4th energy levels of the element in #24 above correct? Explain
3s
3p
4s
3d
40) On the table to the left – color and label these blocks: the s block
(red), the p block (yellow), the d block (green), and the f block (brown)
41) 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
Photons and the Electromagnetic Spectrum
41) An electron that is closest to the nucleus possible (at the lowest energy level possible) is said to be in its
___________ _________________.
42) When an electron jumps up to a higher energy level and then falls back to its ground state a ___________ is released.
43) 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-variable/specific-quantized)
amount of energy.
44) The color spectra (types of colors produced) of a star can be used to identify the types of ______________ present
in the star.
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