The Periodic Table

Open Ended

Why do you think organizing elements in a table is important for scientists and chemists?

Multiple Choice

Who grouped elements into triads based on their similar properties in 1829?

• John Dalton

• J.W. Dobereiner

• Dmitri Mendeleev

• Marie Curie

Multiple Choice

Who published the first widely recognized periodic table of elements in 1869?

• Dmitri Mendeleev

• John Dalton

• Henry Moseley

• Marie Curie

Open Ended

Compare how elements were organized in Mendeleev's periodic table and in the modern periodic table.

Open Ended

Explain why some elements from period 6 and 7 are placed beneath the periodic table.

Multiple Choice

What are the three classes of elements according to the periodic table?

• Metals, Nonmetals, Metalloids

• Metals, Gases, Liquids

• Solids, Liquids, Gases

• Metals, Noble Gases, Halogens

Multiple Select

Which of the following are properties of metals?

• Good conductors of heat and electricity

• High luster or sheen

• All are gases at room temperature

• Most are malleable and many are ductile

Multiple Choice

Which of the following statements about nonmetals is correct?

• Most nonmetals are good conductors of electricity.

• All nonmetals are solids at room temperature.

• Most nonmetals are gases at room temperature.

• Nonmetals are usually found in the lower left corner of the periodic table.

Open Ended

Explain how the properties of metalloids can be controlled and provide an example based on the images.

Multiple Choice

How do metalloids differ from metals and nonmetals in terms of their electrical conductivity?

• Metalloids are always good conductors of electricity.

• Metalloids never conduct electricity.

• Metalloids can conduct electricity under certain conditions.

• Metalloids are always insulators.

Multiple Choice

Based on the periodic table diagram, which section contains the metalloids?

• Transition Metals

• Noble Gases

• Between Nonmetals and Metals

• Rare Earth Metals

Multiple Choice

Which direction on the periodic table does atomic radius increase, and which direction does it decrease?

• Increases down a group, decreases across a period

• Increases across a period, decreases down a group

• Increases diagonally, decreases vertically

• Increases only for noble gases

Multiple Choice

Which of the following statements best describes an ion?

• An atom or group of bonded atoms with a positive or negative charge

• A neutral atom

• An atom that only loses electrons

• A molecule with no charge

Multiple Select

Select all the correct trends for ionization energy in the periodic table.

• Increases across a period

• Decreases down a group

• Decreases across a period

• Increases down a group

Open Ended

How does electron affinity generally change as you move across a period and down a group in the periodic table?

Multiple Choice

Which of the following statements best describes electron affinity?

• It is the energy released when a neutral atom acquires an electron.

• It is the energy required to remove an electron from an atom.

• It is the energy required to split a molecule into atoms.

• It is the energy released when two atoms bond together.

Open Ended

Explain how the number of valence electrons in an element's group relates to its chemical reactivity.

Multiple Choice

Which property listed is a measure of how strongly an atom attracts electrons in a chemical bond?

• Atomic Radius

• Electronegativity

• Valence Electrons

• Metallic Character

Multiple Choice

What trend in electronegativity is observed as you move from left to right across a period in the periodic table?

• Electronegativity increases

• Electronegativity decreases

• Electronegativity remains constant

• Electronegativity first increases then decreases

Multiple Choice

Which statement best explains why metals tend to lose electrons in chemical reactions?

• They have low ionization energies.

• They have high electronegativity.

• They have a full outer shell.

• They have high electron affinity.