Periodic TRENDS REVIEW (plus more!)

It refers to the net pull of the nucleus to the valence electrons or outer electrons.

• Nuclear charge

• Effective nuclear charge

• Electron shielding

• Number of protons

Tags

NGSS.HS-PS1-8

Which of the following best defines the term first ionization energy?

• The energy released when an electron is removed from a gaseous atom.

• The energy required to remove an electron from a gaseous atom.

• The energy released when a gaseous atom gains an electron.

• The energy required to add electrons to gaseous atoms.

Which of the following properties increases across the period (left to right)?

• Electron shielding

• Atomic radius

• Effective nuclear charge

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Potassium and sodium are both alkali metals. Why is the atom of potassium bigger than the atom of sodium?

• It has more energy levels.

• It has greater number of protons.

• It has less electron shielding.

• It has higher effective nuclear charge.

Tags

NGSS.HS-PS1-1

Identify a property of Group 1 elements that increase down the group (top to bottom). NOTE: Check ALL possible correct answers.

• Effective nuclear charge

• Ionization energy

• Electron Shielding

• Atomic Radius

Which of the following groups of elements do you expect to have the highest ionization energy?

• Alkali Metals

• Noble Gases

• Halogens

• Transition metals

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following species will you expect to have the biggest ionic radius?

• Sr²⁺

• Te²⁺

• I^-

• Cs⁺

S and Cl are on the same period. Why will the ionization energy of Cl be higher than S?

• S has a higher effective nuclear charge.

• Cl has higher effective nuclear charge.

• S has greater electron shielding.

• Cl has greater electron shielding.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2