Study Guide for Periodic Table Test
Students should be able to:
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Define the terms group and period
Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements
Describe the differences between metals and non-metals
Use proton number and the simple structure of atoms to explain the basis of the Periodic Table, with special
reference to the elements of proton number 1 to 20
Deduce the electron configuration of an atom from the element’s position on the periodic table, and vice versa.
Explain periodic trends across periods and down groups including; reactivity, metallic properties, atomic
number, atomic radii, ionization energy, and electronegativity.
Explain why noble gases are unreactive.
Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic
structures and of valence electrons (the ideas of the distribution of electrons in s and p orbitals and in d block
elements are not required.)
Relate the properties of the main-group elements to their electron arrangements.
Predict how an atom's electron arrangement influences its ability to transfer or share electrons and is related its
position on the periodic table.
Relate trends in the periodic table to the atomic structures of elements.
Practice Questions: NOTE: These are just a sample. You can make your own questions based on the learning objectives
above!
1. Define the following terms; group, period, electronegativity, ionization energy, luster, malleable, ductile, atomic
radii, ion, oxidation number, valence electron, valence shell, octet rule, cation, anion
See Posted Powerpoint presentations
2. Draw the Bohr models for a Calcium atom and a Calcium ion. Then explain which has the larger atomic radii
based on what you know about atomic structure.
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The larger atomic radii is the calcium atom because it has an extra energy level to hold the 2 valence electrons.
When the ion forms the 2 valence electrons are given away decreasing the size of the ion by one energy level.
3. Complete the following table:
Element
Number of Energy Levels
Number of Valence Electrons
Electron Configuration Using
Noble Gas
4
3
[Ar], 3
5
4
[Kr], 4
7
2
[Rn], 2
5
8
[Xe]
5
5
[Kr],5
6
6
[Xe], 6
Gallium
Tin
Radium
Xenon
Antimony
Polonium
4. Describe everything you know about Strontium based on the periodic table.
Atomic number 38, Atomic mass 87.62 g/mol, 38 protons, 50 neutrons, 38 electrons, 5 energy levels, 2 valence
electrons, a metal, solid at room temperature, good conductor, high melt/boiling points, high density,
malleable (flattens when hammered), ductile (pulls into a wire), lustorous (shiny), member of the alkaline
earth element family, relatively reactive, oxidation number of +2, gives away two valence electrons, reacts
readily with halogens and oxygen family, forms salts when bonded with a halogen, found in Earth’s crust,
more reactive than calcium but less reactive than barium.
5. What properties would you expect Selenium to have? Why?
Selenium is a member of the oxygen family. It has 4 energy levels and 6 valence electrons. Selelnium is a nonmetal so does not conduct heat or electricity well. It also has a low density and low melting/boiling points.
Selenium forms a anion with an oxidation number of -2 when it accepts electrons. It has a high
electronegativity because it only needs two valence electrons to have a full shell.
6. What are metalloids? What properties do they have? Identify all the metalloids on the Periodic Table.
Metalloids are elements that lie along the zigzag line on the periodic table starting with Boron and moving
down in steps. These elements share properties of both metals and non-metals. These are good
semiconductors. The metalloids include: Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, and
Polonium
7. List the properties of the following families; noble gases, transition metals, carbon family, alkali metals,
halogens, alkaline earth metals
See Powerpoint on mrspage.com
8. In lab you are testing the properties of an unknown element. You have made the following observations:
 The element is a solid at room temperature
 The element reacts readily with water
 The element is soft enough to cut with a knife
 The element has a mass greater than argon but lower than krypton
 The element forms a salt when it reacts with a halogen
Based on these observations, predict which element you believe you are testing? What other properties would
this element have?
Potassium: high melting/boiling points, high density, extremely reactive, oxidation number = +1, not found
unbonded, lustrous, malleable, ductile, reacts readily with oxygen in air (oxidizes quickly)
9. Explain why Silicon is likely to share its electrons while radium is more likely to form an ion.
Silicon is in the carbon family and has 3 energy levels and 4 valence electrons. Since its valence shell is half
full, it is not energetically favorable to gain 4 or lose 4 electrons. For this reason silicon will most often fill it’s
valence shell by sharing electrons with another element. Radium however is in group 2, alkaline earth metals.
This element has 7 energy levels and 2 valence electrons. The two valence electrons makes radium unstable.
In addition these electrons are far from the nucleus and therefore have a lot of shielding. This lowers the
electromagnetic force between the valence electrons and the protons in the nucleus. This makes radium very
reactive and it will easily give away its two valence electrons in order to fulfill the octet rule.
10. Complete the following table:
See Powerpoint for why
Trend
Increasing or WHY??
Decreasing
increasing
Valence Electrons
Across Period
increasing
Energy Levels
Down Group
decreasing
Across Period
Metallic Properties
increasing
Down Group
Across Period
Reactivity
Decreases
from groups
I & VII
towards
center
Increases
Down Group
Decreases
Across Period
Atomic Radii
Increases
Down Group
Decreases
Across Period
Ionization Energy
Increases
Down Group
Across Period
Electronegativity
Down Group
Increases
(ignoring
noble gases)
Decreases