Periodic table trends review

Moseley discovered that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing

• atomic mass

• density

• radioactivity

• atomic number

As the atomic number increases within a group (top to bottom), the atomic radius

• generally increases

• remains generally constant

• decreases regularly

• varies unpredictably.

The halogens are located on the periodic table in Group

• 1

• 2

• 17

• 18

The number of valence electrons for Group 2 elements is

• 2

• 8

• n-1

• equal to the period number

The electron configuration of an element in its ground state is [Ar]3d ^{1 0} 4s ² 4p ⁵ . This element is in the _______________________period.

• second

• third

• fourth

• no correct answer

The electrons available to be gained, lost, or shared in the formation of chemical compounds are called _______________________.

One-half the distance between the nuclei of identical atoms that are bonded together is the _______________________.

Of the following elements, which has the largest atomic radius: sodium (atomic number 11), magnesium (atomic number 12), phosphorus (atomic number 15), and chlorine (atomic number 17). Explain your answer in terms of trends in the periodic table.

In the space provided, identify the period and block to which each of the following elements belongs.

Krypton: 1s ² 2s ² 2p ⁶ 3s ² 3p ⁶ 3d ¹⁰ 4s ² 4p ⁶ ____________________________________________

The periodic law states that

• no two electrons with the same spin can be found in the same place in an atom

• the physical and chemical properties of the elements are functions of their atomic number

• wave patterns repeat at regular intervals

• the chemical properties of elements can be grouped according to periodicity