Investigation 5 Practice Test

In the 1860s, Dmitri Mendeleev designed a Periodic Table of elements based on extensive research and observations. He left several gaps in his Periodic Table for elements that had yet to be discovered. A section of a Periodic Table with one such gap is shown above. Which of the following sets of data could match the unknown element?

• Non-metal, Mass: 72

• Metalloid, Mass: 78

• Reactive metal, Mass: 71

• Metalloid, Mass: 74

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Which of the following describes the properties of noble gases?

• They have high boiling points.

• They are highly reactive.

• They are generally unreactive.

• They are solid at room temperature.

Which family correctly represents the elements in Group 1 on the Periodic Table?

• Transition metals

• Alkali metals

• Lanthanide elements

• Actinide series

Some physical properties of elements in a group of the periodic table are described above. The elements described above belong to which group?

• Alkaline earth metals

• Noble gases

• Alkali metals

• Halogens

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The number of valence electrons in Group 2 elements is —

• 0

• 1

• 2

• 3

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The reactivity trends on the Periodic Table depends on valence electrons. What family on the Periodic Table is

identified as the most reactive nonmetals?

• 1

• 12

• 13

• 17

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From which of the following atoms would it be the most difficult to remove an electron?

• Sodium

• Aluminum

• Sulfur

• Chlorine

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Using the Periodic Table, predict which elements will have similar chemical properties or reactivity.

• Cadmium, calcium, and carbon

• Magnesium, strontium, and barium

• Rubidium, yttrium, and zirconium

• Nitrogen, sulfur, and bromine

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Alkali metals react very readily with halogens and form ionic compounds such as table salt (NaCl) and many

others. Which of the following explanations most completely describes why these two families of elements reacts readily?

• Alkali metals are negative and halogens are positive, so they attract each other.

• The alkali metals have one valence electron, and the halogens are one short of an octet.

• Alkali metals and halogens can very easily share eight valence electrons between them.

• The halogens very easily donate valence electrons to the alkali metals so that all have eight.

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As the atomic number increases within a group of elements, the atomic radius usually —

• decreases

• remains the same as the one above it

• increases

• decreases, then increases