Honors Chemistry Unit 3 Practice Quizizz

How does electronegativity change as you move from top to bottom in a group on the periodic table?

• Generally decreases

• Generally increases

• Remains the same

• Not enough information to determine

Answer explanation

Electronegativity generally decreases as you move from top to bottom in a group on the periodic table due to the increasing distance between the nucleus and the valence electrons, which reduces the nucleus's ability to attract electrons.

Which element is likely to have the lowest ionization energy?

• Helium

• Neon

• Potassium

• Argon

Answer explanation

Potassium has the lowest ionization energy among the options because it is in Group 1 of the periodic table, where elements have larger atomic radii and less nuclear charge holding the outermost electron, making it easier to remove.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following elements has the highest ionization energy?

• Fluorine

• Chlorine

• Neon

• Helium

Answer explanation

Helium has the highest ionization energy among the given elements due to its small atomic size and full electron shell, making it more difficult to remove an electron compared to Fluorine, Chlorine, and Neon.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which group on the periodic table is known for having two valence electrons?

• group 2

• group 1

• group 18

• group 17

Answer explanation

Group 2 on the periodic table, also known as the alkaline earth metals, is characterized by having two valence electrons. This distinguishes it from groups 1, 17, and 18, which have one, seven, and eight valence electrons, respectively.

Tags

NGSS.HS-PS1-1

Which of the following elements is classified as a halogen?

• Br

• He

• Ne

• Cu

Answer explanation

Br (bromine) is classified as a halogen, which are elements in Group 17 of the periodic table. He (helium) and Ne (neon) are noble gases, while Cu (copper) is a metal. Thus, Br is the correct choice.

Elements in group 1 are characterized by having ___________ in their outermost shell.

• two electrons

• eight electrons

• one electron

• seven electrons

Answer explanation

Elements in group 1, known as alkali metals, have one electron in their outermost shell. This single electron makes them highly reactive and is a defining characteristic of this group.

Tags

NGSS.HS-PS1-1

Determine the period and group of the element with the electron configuration [Ar]4s²3d¹⁰4p⁵.

• period 4, group 17

• period 4, group 2

• period 3, group 16

• period 4, group 15

Answer explanation

The electron configuration [Ar]4s²3d¹⁰4p⁵ indicates the element is in period 4 (4th energy level) and has 7 valence electrons (4p⁵), placing it in group 17 (the halogens). Thus, the correct answer is period 4, group 17.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Elements in the same group exhibit similar _________.

• chemical properties

• atomic mass

• electron affinity

• ionization energy

Answer explanation

Elements in the same group of the periodic table have similar chemical properties due to their similar valence electron configurations, which influence their reactivity and bonding behavior.

Tags

NGSS.HS-PS1-2

What is the electron configuration of the element in group 14 and period 3 of the periodic table?

• [Ne]3s²3p²

• [He]2s²2p²

• [Ar]4s²3d¹⁰4p²

• [Kr]5s²4d¹⁰5p²

Answer explanation

The element in group 14 and period 3 is silicon (Si). Its electron configuration is [Ne]3s²3p², indicating it has 2 electrons in the 3s subshell and 2 in the 3p subshell, which matches the correct choice.

Tags

NGSS.HS-PS1-1

Where on the periodic table would you expect to find elements with the smallest atomic radii?

• lower left

• lower right

• upper right

• upper left

Answer explanation

Elements with the smallest atomic radii are found in the upper right of the periodic table. This is due to increased nuclear charge and decreased electron shielding, which pull electrons closer to the nucleus.

Tags

NGSS.HS-PS1-1