Periodic Table Trends Worksheet
Explore and understand key periodic table trends including atomic radius, ionization energy, electronegativity, and metallic character for Grade 10 Chemistry students.
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Periodic Table Trends
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Read each question carefully and answer to the best of your ability. Use your knowledge of periodic table trends to explain your reasoning.
1. Which of the following elements has the largest atomic radius?
Lithium (Li)
Fluorine (F)
Cesium (Cs)
Neon (Ne)
2. Which trend describes the increase in ionization energy across a period?
Electrons are added to new energy levels.
Nuclear charge increases, pulling electrons closer.
Shielding effect becomes more significant.
The number of valence electrons decreases.
1. is a measure of the ability of an atom in a chemical compound to attract electrons.
2. As you move down a group in the periodic table, the atomic radius tends to .
3. Elements with high electronegativity and high ionization energy are typically .
1. Metallic character generally increases from left to right across a period.
True
False
2. Ionization energy is the energy required to remove an electron from a gaseous atom.
True
False
1. Explain why atomic radius decreases across a period.
2. Describe the trend of electronegativity down a group and explain the reason behind it.
Reference the periodic table below to answer the questions.
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