Periodic Table Trends

Multiple Choice

Which of the following best describes a periodic trend in the periodic table?

• A pattern in the properties of elements as you move across a period or down a group

• A random change in element properties

• A trend that only occurs in metals

• A trend that only occurs in nonmetals

Multiple Choice

Which property is NOT listed as a periodic property in the first image?

• Atomic Radius

• Ionic Radius

• Electronegativity

• Melting Point

Multiple Choice

What is the definition of atomic radius?

• The distance between two atoms

• Half the distance between nuclei of identical atoms

• The size of the nucleus

• The number of electrons in an atom

Open Ended

Explain why atomic radius decreases as you move across a period in the periodic table.

Open Ended

What causes the atomic radius to increase as you move down a group?

Multiple Select

Which of the following statements about atomic radius trends is/are correct?

• Atomic radius increases as you move down a group

• Atomic radius decreases as you move across a period

• Valence electrons are shielded from nuclear charge

• Outermost orbital size increases down a group

Multiple Choice

Which factor causes the overall atomic radius to become larger?

• More inner electrons shield the outer electron from the nucleus

• The nucleus attracts the outer electron more strongly

• Electrons are lost from the atom

• Atoms gain protons

Open Ended

Explain how the loss or gain of electrons affects the charge of an atom and its classification as an ion.

Multiple Choice

Which of the following statements about positive ion (cation) formation is correct?

• The radius becomes larger when an atom loses electrons

• Electrostatic repulsion increases when an atom loses electrons

• The loss of a valence electron can result in a smaller radius

• Atoms gain electrons to form cations

Open Ended

Describe the trend in ionic radius as you move left to right across a period for both positive and negative ions.

Multiple Choice

Which statement best describes ionization energy?

• The energy required to add an electron to an atom in the gas phase.

• The energy required to remove an electron from an atom or ion in its ground state in the gas phase.

• The energy released when an atom gains an electron.

• The energy needed to break a chemical bond.

Open Ended

What is the periodic trend in ionization energy? Why?

Multiple Select

Which of the following statements about ionization energy trends is/are correct?

• Ionization energy increases as you move across a period.

• Ionization energy decreases as you move down a group.

• Ionization energy remains constant across a period.

• Ionization energy decreases as you move across a period.

Multiple Choice

Based on the table, which element in Period 2 has the largest jump in ionization energy between its second and third ionizations?

• Lithium (Li)

• Beryllium (Be)

• Boron (B)

• Carbon (C)

Open Ended

Explain how the diagram in the last image illustrates the trend in first ionization energies across the periodic table.

Multiple Choice

Which element is assigned the highest value of electronegativity on the Pauling scale?

• Oxygen

• Fluorine

• Chlorine

• Nitrogen

Open Ended

Explain the periodic trends in electronegativity and the reasons behind these trends.

Multiple Select

Select all elements that have electronegativity values greater than 3.0 according to the Pauling scale.

• Fluorine

• Oxygen

• Nitrogen

• Chlorine

Open Ended

How do periodic trends help scientists predict the behavior of elements?