Atomic Radius
Which element has a higher ionization energy: Na or Mg?
Mg
Which element has a higher ionization energy: Na or Mg?
Mg
Which element has the highest electronegativity on the periodic table?
Fluorine
Is Beryllium a metal or nonmetal?
Metal
Which element is larger: Br or Br-?
Br-
Does atomic radius increase or decrease as you move across a period?
Decrease
Does ionization energy generally increase or decrease as you go down a group?
Decrease
Does electronegativity generally increase or decrease across a period?
Increase
Which side of the periodic table contains metals?
Left side
Does atomic radius increase or decrease as you move down a group?
Increase
Arrange these elements in order of increasing atomic radius: Li, Be, B.
B < Be < Li
Rank these elements by ionization energy (highest to lowest): F, Li, B.
F > B > Li
Compare the electronegativity of Oxygen and Sulfur.
Oxygen has a higher electronegativity than Sulfur.
Name one property of metals and one of nonmetals.
Metals are good conductors of electricity, while nonmetals are poor conductors.
Which has the higher ionization energy: Oxygen or Fluorine?
Fluorine
Compare the atomic radius of Na and Na+
Na+ has a smaller radius than Na.
Why is ionization energy lower for alkali metals than for noble gases?
Alkali metals have fewer protons attracting their outer electrons, making it easier to remove an electron.
Explain why noble gases do not have electronegativity values.
Noble gases generally do not form bonds, so they do not attract electrons in bonding situations.
What do we call elements with properties of both metals and nonmetals?
Metalloids
Explain why atomic radius increases down a group.
As you move down a group, more electron shells are added, increasing the size of the atom.
Arrange these elements in order of decreasing atomic radius: Cl, S, P, Al.
Al > P > S > Cl
Explain why ionization energy increases across a period.
As protons increase across a period, the nuclear charge increases, pulling electrons closer and making them harder to remove.
Arrange these elements by increasing electronegativity: Cl, F, Br, I.
I < Br < Cl < F
Why do metals tend to lose electrons and form cations?
Metals have lower ionization energies and want to achieve a stable electron configuration by losing electrons.
Which group has elements with the highest electronegativity values?
Group 17 (Halogens)