Applied Chemistry
Study Guide
Periodic Table
Name __Answer Key_________________________
Date __________________
Period ______
1. Who is responsible for developing the first periodic table? _Dimitri Mendeleev____________
Describe how he organized elements (2 strategies):
-Arranged elements in order of increasing atomic mass
-Sorted elements with similar chemical properties together into groups
2. Be able to find the group number, period number, number of valence electrons, and most likely ion for
any element in the periodic table.
Element
Group
Number
Period
Number
Number of Valence
Electrons
Most Likely Ion
Strontium
2
5
2
Sr​+2
Gallium
13
4
3
Iodine
17
5
7
Argon
18
3
8
Hydrogen
1
1
1
Carbon
14
2
4
I​-1
H​+1
3. Be able to draw electron dot diagrams. Example: Oxygen
Calcium
Lithium
Neon
Phosphorus
Fluorine
Aluminum
4. State the octet rule and explain how it is used to determine what ion an element will form.
Elements gain, lose, or share electrons until atoms have a full valence shell with 8 electrons. Atoms
that have almost 8 electrons (6 or 7) will add electrons to get to 8 and will form negative anions. Atoms
that have only a couple of valence electrons (1 or 2) will lose those electrons so that the next energy
level down has 8 electrons. This forms positive cations.
5. Recognize and label the location on the periodic table of the following groups of elements:
Metals, Nonmetals, Metalloids, Alkali metals, Alkaline earth metals, Transition metals, Lanthanides,
Actinides, Halogens, Noble gases
6. Describe the properties of metals (list as many as possible).
-solid, hard
-shiny
-malleable, ductile
-conductors for heat and electricity
-high melting and boiling points
-react with acid
-tend to rust in air
-form cations
7. Describe the properties of nonmetals (list as many as possible).
-most are solid or gas
-dull
-brittle
-low melting and boiling point
-poor conductors of heat and electricity
-form anions
8. Compare and contrast the properties of the alkali metals and the alkaline earth metals (2 similarities
and 2 differences).
Both groups of metals contain elements that are silvery-white solids, good conductors, and very
malleable. Alkali metals react violently with water and form +1 cations. Alkaline earth metals are less
reactive (react more slowly with water and react with acid) and form +2 cations.
9. How are the elements in the halogen group similar to each other? How are they different?
All the halogen elements are highly reactive, have 7 valence electrons, and form -1 anions. They have
very different physical properties at room temperature: two are greenish-yellow gases, one is a brown
liquid, and another is a purple solid.
10. How does atomic size change across a period of elements (left to right)? How does size change within
a group (top to bottom)?
Atomic size decreases across a period (from left to right) and increases down a group (top to bottom).
11. Choose 4 elements from period 5 and list them in order from smallest to largest.
Answers will vary. Check to make sure your response is consistent with the trend from #10.
12. What is ionization energy? Describe the periodic trends for ionization energy (how this property
changes across a period and down a group).
Ionization energy is the energy required to remove an electron from an atom. Ionization energy
increases across a period (left to right) and decreases down a group (top to bottom).
13. Complete the sentence by circling the correct word from the pair: When an atom loses an electron,
there is less repulsion between the remaining electrons, so ( c
​ ations​ / anions ) , which have a
(​positive​ / negative ) charge are ( ​smaller​ / larger ) than neutral atoms of the same element.
14. Complete the sentence by circling the correct word from the pair: When an atom gains an electron,
there is more repulsion between the remaining electrons, so ( cations / ​anions​ ) , which have a
(positive / ​negative​ ) charge are ( smaller / ​larger​ ) than neutral atoms of the same element.
15. List the three types of compounds, and describe what types of elements come together to form each
type of compound.
Ionic - compound of a metal and a nonmetal
Covalent - compound of only nonmetals
Metallic - compound of only metals
16. Label each property as being true for ionic, covalent, or metallic compounds (some properties may be
true for more than one type of compound).
a. Conduct electricity when dissolved in water
Ionic
b. Low melting point
Covalent
c. High boiling point
Covalent, metallic
d. Conduct electricity as a solid
Metallic
e. Typically does not dissolve in water
Covalent, Metallic
17. Label each compound as ionic or covalent.
a. KCl
Ionic
b. NH​3 Covalent
c. CO
Covalent
d. NaF Ionic
e. MgO Ionic
18. Draw a sketch of the electron sea model of metallic bonding.
19. Describe the different ways that valence electrons are used to form ionic compounds, covalent
compounds, and metallic compounds.
In ionic compounds, valence electrons are transferred from the metal to the nonmetal. In covalent
compounds, electrons are shared between the atoms. In metallic compounds, electrons flow freely
(“sea of electrons”) among the metal nuclei.