Atomic Radius
Ionization Energy
Electronegativity
Types of Bonds
IMF
100

Which element has a larger atomic radius, Sodium (Na) or Magnesium (Mg)?

Sodium

100

What ionization energy?

The energy required to remove an electron from an

atom in its gaseous state

100

Define electronegativity.

The tendency of an atom to attract electrons in a chemical bond. 

100

What type of bond forms when electrons are shared equally between atoms?

Nonpolar covalent bond

100

What type of IMF (Intermolecular force) is present in all molecules?

London dispersion forces


200

Does the atomic radius increase or decrease as you move down a group on the periodic table?

Increase

200

Which has a higher ionization energy, Helium (He) or Lithium (Li)?

Helium (He)

200

Which element has the highest electronegativity?

Fluorine (F)


200

What type of bond forms between metals and nonmetals?

Ionic bond

200

Which is stronger: hydrogen bonds or London dispersion forces?

Hydrogen bonds

300

Why does the atomic decrease across a period?

the increase in nuclear charge

300

What happens to ionization energy as it moves down a group?

It decreases
300

What happens to electronegativity as you move from left to right across a period?

It increases

300

Why do polar covalent bonds have partial charges?

Electrons are shared unequally = dipole moment

300

What are dipole-dipole interactions?

IMFs that occur between molecules with permanent dipoles.

400

Which has a larger atomic radius, Chlorine (Cl) or Bromine (Br).

Bromine (Br)

400

Why does ionization energy increase across a period?

Because of the increased nuclear charges

400

Why does electronegativity decrease down a group?

The increased distance from the nucleus and electron shielding 

400

Give an example of a molecule with a polar covalent bond

H2O

400

Which of the following molecules will have hydrogen bonding: CH4, H2O, NH3?


H2O and NH3

500

Explain why noble gases are not included in trends for atomic radius across a period.

They have a full valence shell and do not form bonds
500

Why does oxygen have a lower first ionization energy than nitrogen?

The electron repulsion in the p-orbitals makes it easier to remove an electron from oxygen.
500

Why do noble gases generally not have electronegativity values?

They do not form bonds due to having a full valence shell

500

How do electronegativity differences deter the type of bond (ionic, polar covalent, nonpolar covalent)?

A large electronegativity difference leads to ionic bonds (>1.7)

Moderate difference leads to polar covalent bonds (0.4-1.7)

Small/no difference leads to nonpolar covalent bonds (<0.4)

500

Explain why water has a higher boiling point than methane (CH4). 

Water has strong hydrogen bonding, while methane only has weak London dispersion forces