Chapter 7 Periodic Trends

As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 

• the number of protons(Z_eff) increases, so attraction to electrons increases

• the number of energy levels increases
• the number of electrons increases
• the atomic mass increases

Francium (Fr) has the lowest ionization energy in Group 1 because - 

• it has the smallest number of valence electrons
• it has the greatest atomic mass
• it has the greatest number of protons, so it attracts its electrons the strongest
• its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

The element with the smallest ionization energy in Period 6 is - 

• Rn
• Cs
• Os
• Tm

The energy required to remove electrons is the definition of: 

• Electronegativity
• Atomic Number
• Atomic Radius
• Ionization energy

Electronegativity is...

• the ability of an atom to attract electrons

• the ability of an atom to lose electrons
• the energy required to remove an electron from a specific atom
• how easy it is to make friends. 

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

Which periodic group has the smallest atomic radius?

• Alkali metals
• Halogens
• Noble Gases
• Transition metals

Which of the following will have a higher ionization energy than arsenic (As)?

• Gallium (Ga)
• Neon (Ne)
• Antimony (Sb)
• Germanium (Ge)

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)
• Neon (Ne)
• Antimony (Sb)
• Germanium (Ge)

Which of the alkaline-earth metals has the smallest electronegativity

• Be

• Sc

• Ra

• Sr