Atomic Radius
Which element has a larger atomic radius, Sodium (Na) or Magnesium (Mg)?
Sodium
What ionization energy?
The energy required to remove an electron from an
atom in its gaseous state
Define electronegativity.
The tendency of an atom to attract electrons in a chemical bond.
What type of bond forms when electrons are shared equally between atoms?
Nonpolar covalent bond
What type of IMF (Intermolecular force) is present in all molecules?
London dispersion forces
Does the atomic radius increase or decrease as you move down a group on the periodic table?
Increase
Which has a higher ionization energy, Helium (He) or Lithium (Li)?
Helium (He)
Which element has the highest electronegativity?
Fluorine (F)
What type of bond forms between metals and nonmetals?
Ionic bond
Which is stronger: hydrogen bonds or London dispersion forces?
Hydrogen bonds
Why does the atomic decrease across a period?
the increase in nuclear charge
What happens to ionization energy as it moves down a group?
What happens to electronegativity as you move from left to right across a period?
It increases
Why do polar covalent bonds have partial charges?
Electrons are shared unequally = dipole moment
What are dipole-dipole interactions?
IMFs that occur between molecules with permanent dipoles.
Which has a larger atomic radius, Chlorine (Cl) or Bromine (Br).
Bromine (Br)
Why does ionization energy increase across a period?
Because of the increased nuclear charges
Why does electronegativity decrease down a group?
The increased distance from the nucleus and electron shielding
Give an example of a molecule with a polar covalent bond
H2O
Which of the following molecules will have hydrogen bonding: CH4, H2O, NH3?
H2O and NH3
Explain why noble gases are not included in trends for atomic radius across a period.
Why does oxygen have a lower first ionization energy than nitrogen?
Why do noble gases generally not have electronegativity values?
They do not form bonds due to having a full valence shell
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)
Explain why water has a higher boiling point than methane (CH4).
Water has strong hydrogen bonding, while methane only has weak London dispersion forces