Chemistry I Unit 7, the Periodic Table
Chemistry I – Unit 7, The Periodic Table
Chapter 6 The Periodic Table
Section / Pages / Homework6.1- Organizing the elements / 155 – 160 / Page 160 # 2, 3, 5, 6
6.2- Classifying the elements / 161 – 167 / Page 167 # 13, 14
6.3- Periodic trends / 170 – 178 / Page 178 # 22, 23
Review / 181 / 33, 35, 36, 38, 39, 42, 43, 49, 52
Using the periodic table below label the following areas:
Alkali metals Noble gases Transition metals Halogens Alkaline earth
Lanthanide series Actinide series main group/representative elements Group numbers
Period numbers
List 3 elements from each of the following groups and list two properties:
From each of the following groups, list a) 3 elements and b) two properties of that group
1) Noble gases
2) Halogens
3) alkali metals
4) alkaline earth metals
5) transition metals
PERIODIC TRENDS:
Atomic Radius
Define atomic radius
How do the sizes of atoms change as you move across a period? Why?
How do the sizes of atoms change as you move down a group? Why?
Ionization energy:
Define ionization energy
How does ionization energy change across a period? Why?
How does ionization energy change down a group? Why?
Electronegativity:
Define electronegativity
How does electronegativity change across a period? Why?
How does electronegativity change down a group? Why?
What is the most electronegative element?
Why are there no values for electronegativity for the Noble gases?
Metallic character
How does metallic character of the elements change across and down the periodic table?
Ionic Radius
How does the size of an atom change when it gains electron(s) and forms an anion (negative ion)?
How does the size of an atom change when it loses electron(s) and forms a cation (positive ion)?
Periodic Trends
1) Circle the element in each pair with the largest atomic radius:
a) Li or Rb / b) Li or B / c) F or In2) Circle the element in each pair with greatest ionization energy
a) Na or Cs / b) Na or Cl / c) F or Ca3) Circle the element in each pair with the greatest eletronegativity
a) F or I / b) Li or C / c) Mg or Ba4) Circle the element in each pair with the larger atomic radius
a) Na or Na+1 / b) Br or Br -1 / c) Al+3 or S –25) Rank the following row (going across) of 3 elements in order of increasing atomic radius (smallest to largest)
a) F / b) Li / c) Bea) Mg / b) Cl / c) Si
a) Te / b) S / c) O
6) Rank the following row (going across) of 4 elements in order of increasing ionization energy
a) Ge / b) C / c) Sn / d) Sia) Br / b) K / c) As / d) Ge
a) O / b) K / c) Si / d) F
7) Rank the following row (going across) of 4 elements in increasing electronegativity
a) Ca / b) K / c) Se / d) Bra) Br / b) I / c) Cl / d) F
a) Rb / b) Li / c) Na / d) Fr
Use the letters in the Periodic Table below to answer the following questions:
A AB
/ C / DE
/ F / G / HI / J / K / L
M / N
O / * / P / Q
**
* / R
** / S
8) Which letter represents the most reactive alkali metal? ______
9) Which letter represents a metal in the actinide series? ______
10) Which letter represents a nonmetal that is not a member of the halogen family in the 3rd period? ______
11) Which letter represents a diatomic element in the 2nd period? ______
12) Which letter represents an element that is dull, brittle and a solid in the 2nd period? ______
13) Which letter represents an alkaline earth metal? ______
14) Which letter represents an element that would have 5s25p5 as its valence shell electron configuration? ______
15) Which letter represents an element, in the third energy level, whose most common oxidation # is –1? _____
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Review Questions
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