Periodic Trends, Ions and Formulas

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 atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Which of the following will have a lower ionization energy than Scandium (Sc)?

• Helium (He)
• Titanium (Ti)
• Calcium (Ca)
• Magnesium (Mg)

Atoms that have a high electronegativity, _______________.

• give up their electrons more easily.

• hold on to electrons more tightly.

• have more electron shells.

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

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

• decreases, increases 
• increases, increases
• increases, decreases 
• stays the same, increases

Atomic radius generally increases as we move __________.  

• down a group and from right to left across a period 
• up a group and from left to right across a period 
• down a group and from left to right across a period 
• up a group and from right to left across a period 

Which of the following pairs of elements have similar properties

• Barium and Calcium
• Sodium and Magnesium
• Nickel and Copper
• Lithium and Helium 

The tendency of an atom to attract electrons and acquire a negative charge

• electronegativity
• charge
• bonding ability
• electron configuration

Which is larger, P or P^-3?

• P

• P^-3

• both are same size