(H) Periodic Table Test Review

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each element....

• decreases

• increases

• remains the same

• none of the above

Which atom has the largest atomic radius?

• potassium

• rubidium

• francium

• cesium

As you move down the periodic table atoms get bigger. This is because ____________.

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more energy levels

• The atoms have more nuetrons

As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more mass.

• the atoms have less mass

• the atoms have more protons.

• the atoms have less electrons.

Atoms that have a high electronegativity, _______________.

• give up their electrons more easily.
• hold on to their electrons more tightly.
• have more electron shells.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Ionization energy is...

• the energy required to add an electron to a specific atom
• how much energy it takes to remove an electron from an atom
• the energy required to shield the outer electrons from the nucleus
• a measure of the ability of an atom to attract electrons

Tags

NGSS.HS-PS1-2

Metals have the largest -

• atomic radius and electronegativity

• electronegativity and ionization energy

• atomic radius only

• ionization energy and atomic radius

The element with the largest electronegativity in the halogens is -

• At

• F

• Cl

• Br

The element with the lowest electronegativity in Period 3 is -

• Na

• Cl

• Ar

• Mg

The electronegativity of Cl is the highest in Period 3. Why?

• Cl is the largest and has the greatest effective nuclear charge

• Cl is the smallest and has the lowest effective nuclear charge

• Cl is the largest and has the lowest effective nuclear charge

• Cl is the smallest and has the greatest effective nuclear charge