Name ___________________________________________
Date ____________________
Class______________________
Unit 3 – Periodic Properties Study Guide
For this unit you should be able to do all of the following:
1.Explain the development of the Periodic Table
a) Mendeleev (using atomic weights)
b) Moseley (using atomic numbers)
c) Periodic Law: the chemical and physical properties of elements are periodic functions (recurrent
functions) of their atomic numbers
2.Read and explain the Periodic Table:
a)Names and Locations of:
i) Groups (vertical – up and down)
ii) Periods (horizontal – across left to right)
iii) Metals and their general properties: malleable, ductile, shiny, good conductors, lose electrons to
form positive ions
iv) Nonmetals and their general properties: Brittle, no metallic luster, poor conductors, gain electrons to
form negative ions
v) Metalloids: elements sharing some metallic and some nonmetallic properties
vi)“Stairway to 7”: boundary line between metals and nonmetals
vii) Main group elements: groups 1-2 and 13-18 (The “A” groups)
viii) Transition metals: groups 3-12; scandium (Sc) through zinc (Zn) and all below them
ix) Lanthanides: elements 58-71, following lanthanum (La)
x) Actinides: elements 90-103, following actinium (Ac)
xi) Alkali metals (group 1): Li, Na, K, Rb, Cs, Fr. Hydrogen (H) is chemically similar.
xii) Alkaline earth metals (group 2): Be, Mg, Ca, Sr, Ba, Ra
xiii) Halogens (group 17): F, Cl, B, I, At
xiv) Noble or inert gases (group 18): He, Ne, Ar, Kr, Xe, Rn, with complete octets
b) s,p,d,f blocks
i)Write the long hand and short hand electron configuration of elements AND Ions including those with
exceptions to the rules
c) valence electrons
i) definition: outermost shell of electrons that determine chemical properties of an element
ii) be able to determine # of valence electrons for any main group element (A group)
iii) Draw Lewis dot diagrams
iv)Importance of valence electrons to physical and chemical properties
v) The octet rule: atoms are most stable with 8 valence electrons (2 in the first period)
d) Ionization
i) Reason why atoms form ions
ii) Predict what ions will form for an atom based on atom’s position on periodic table
3.Understand Periodic Trends and use these trends to predict properties of atoms
a) Recognize that elements within the same group share similar physical and chemical properties
b) Understand the reason why this occurs
c) General Period Trends
i)Atomic radius
(1) Definition
(2) Know trend (both group and period)
Name ____________________________________________
Date ____________________
Class ____________________
(3) Reason for trend (both group and period) (Coulombic Attraction/ Effective Nuclear Charge)
ii)13
Ionization energy
6
(1) Definition
(2) Basic chemical equation
(3) Know trend (both group and period)
(4) Reason for trend (both group and period) (Coulombic Attraction/ Effective Nuclear Charge)
iii) Electronegativity
(1) Definition
(2) Know trend (both group and period)
(3) Reason for trend (both group and period) (Coulombic Attraction/ Effective Nuclear Charge)
iv) Ion Size
(1) Definition
(2) Be able to compare ion size to parent atom
(3) Be able to explain why there is a difference in size between an ion and its parent atom
(Coulombic Attraction/ Effective Nuclear Charge and Octet Rule)
Study Guide Practice Questions
1.Who is given credit for creation of the Periodic Table?
2.When he was putting the table together, what characteristics did he use to place the elements in order?
3.Does the atomic number increase or decrease as you move from left to right? How much does it change from
one element to the next?
4.The vertical columns on the Periodic Table are called what?
5.Why do elements in the same group have similar chemical properties?
6.The horizontal rows are called what?
7.What states of matter are the metals at when they are at room temperature (solid, liquid, and/or gas)?
8.There are two groups (families) on the Periodic Table that are considered the MOST reactive, what are they
(give name and number)?
9. Using your answer from question 8, how many valence electrons does each of those groups (families) have?
Name ____________________________________________
Date ____________________
Class ____________________
136
10.Na is a very
reactive element in Period 3, what other elements in Period 2 would be considered reactive?
11. Every element in the Carbon group (family) has how many valence electrons?
12. Looking at Group 2 (IIA) which element would be the MOST reactive?
13.If a reaction is going to take place, which Halogen would you expect to react the fastest? Why?
14.List 4 properties of metals
15.If K reacts very violently in water, what you expect Fr to do? Why?
16. Label the numbers and letters in the Periodic Table below
B
A
3
1
6
2
4
5
7
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Date ____________________
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136
Use the information
in the box on the left taken from the periodic table to complete the table on the
right.
7
Atomic Mass
17.
N
Atomic Number
18.
Electron Configuration
19.
Chemical Name
20.
Chemical Symbol
21.
Nitrogen
14.007
[He]2s22p3
For each item in Column A, write the letter of the matching item in Column B.
Column A
Column B
________22. A column on the periodic table
a. metals
________23. A row on the periodic table
b. group
________24. Elements in groups 1, 2, and 13 to 18
c. period
________25. Elements that are shiny and conduct electricity
d. representative elements
________26. Elements in groups 3 to 12
e. transition elements
27. Complete the following table
Common name of
group
Formal group
Number
Number of Valence
Electrons
Reactivity
(low, medium or
high)
Representative
Elements
Li, Na, K
Be, Mg, Ca
F, Cl, Br
He, Ne, Ar
Match the following element characteristics
Column A
Column B
________28. a gas, does not react chemically
with any element
________29. solid, high density, good conductor
of electricity
________30. brittle solid, poor conductor of heat
and electricity
a. Metals
b. Non-Metals
c. Metalloids
________31. brittle solid, poor conducts
electricity somewhat
d. Noble Gas
Name ___________________________________________
Date ____________________
Class______________________
In the space at the left, write true if the statement is true; if the statement is false, change the
italicized word or phrase to make it true.
________32.
There are two main classifications of elements.
________33.
More than three-fourths of the elements in the periodic table are nonmetals.
________34.
Group 1 elements (except for hydrogen) are known as the alkali metals.
________35.
Group 13 elements are the alkaline earth metals.
________36.
Group 17 elements are highly reactive nonmetals known as halogens.
________37.
Group 18 elements are very unreactive elements known as transition metals.
________38.
Metalloids have properties of both metals and inner transition metals.
39. Why do sodium and potassium, which belong to the same group in the periodic table, have similar chemical
properties?
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40. How is the energy level of an element’s valence electrons related to its period on the periodic table? Give an example.
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Use the periodic table to match each element in Column A with the element in Column B that has the
most similar chemical properties.
Column A
Column B
_________ 41 arsenic (As)
a. boron (B)
_________ 42. bromine (Br)
b. cesium (Cs)
_________ 43. cadmium (Cd)
c. chromium (Cr)
_________ 44. gallium (Ga)
d. cobalt (Co)
_________ 45. germanium (Ge)
e. hafnium (Hf)
_________ 46. iridium (Ir)
f. iodine (I)
_________ 47. magnesium (Mg)
g. iron (Fe)
_________ 48. neon (Ne)
h. nitrogen (N)
_________ 49. nickel (Ni)
i. platinum (Pt)
________ 50. osmium (Os)
j. scandium (Sc)
________ 51. sodium (Na)
k. silicon (Si)
________ 52. tellurium (Te)
l. strontium (Sr)
________ 53. tungsten (W)
m. sulfur (S)
________ 54. yttrium (Y)
n. zinc (Z)
________ 55. zirconium (Zr)
o. xenon (Xe)
Name ___________________________________________
Date ____________________
Class______________________
Use your periodic table AND the periodic table below to answer the following questions.
56. Into how many blocks is the periodic table divided? ____________________________________________________
57. What groups of elements does the s-block contain? ____________________________________________________
58. Why does the s-block portion of the periodic table span two groups?
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59. What groups of elements does the p-block contain? ____________________________________________________
60. Why are members of group 18 virtually unreactive?
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61. How many d-block elements are there? ______________________________________________________________
62. What groups of elements does the d-block contain? ____________________________________________________
63. Why does the f-block portion of the periodic table span 14 groups?
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64. What is the electron configuration of the element in period 3, group 16? ____________________________________
Circle the letter of the choice that best completes the statement or answers the question.
65. Atomic radii cannot be measured directly because the electron cloud surrounding the nucleus does
not have a clearly defined
a. charge.
b. mass.
c. outer edge.
d. probability.
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Date ____________________
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136
diagram best represents the group and period trends in atomic radii in the periodic table?
66. Which
a.
c.
b.
d.
67. The general trend in the radius of an atom moving down a group is partially accounted for by the
a. decrease in the mass of the nucleus.
c. increase in the charge of the nucleus.
b. fewer number of filled orbitals.
d. shielding of the outer electrons by inner electrons.
68. A(n) _____________ is an atom, or bonded group of atoms, that has a positive or negative charge.
a. halogen
b. ion
c. isotope
d. molecule
69. An atom becomes negatively charged by
a. gaining an electron.
b. gaining a proton.
c. losing an electron.
d. losing a neutron.
70. Which diagram best represents the relationship between the diameter of a sodium atom and the
diameter of a positive sodium ion?
a.
b.
c.
71. What is ionization energy?
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72. Explain why an atom with a high ionization-energy value is not likely to form a positive ion.
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73. What is the period trend in the first ionization energies? Why?
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Name ____________________________________________
Date ____________________
Class ____________________
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74. What is the group trend in the first ionization energies? Why?
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75. State the octet rule.
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76. What does the electronegativity of an element indicate?
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77. What are the period and group trends in electronegativities?
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