Honors Unit 3 Review: Electrons, Periodic Table, and Trends

Electronegativity is...

• how good an atom is at attracting 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. 

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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

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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 

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Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

As you move from left to right on the periodic table, the number of valence electrons.......

• Increases

• Decreases

• Remains the same

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As you move down a group on the periodic table, the number of valence electrons....

• Increases

• Decreases

• Remains the same

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The common charge on an atom in group 17 would be....

• +1

• +7

• -7

• -1

• 17

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Which of the following reasons explains why there is a decimal for most atomic masses?

• The mass of one atom can have a fraction.

• Since electrons are very small mass they only add a little bit, usually only a decimals worth.

• It is the average mass of all the potential isotopes of an atom.

• Neutrons have a mass of 1.1 meaning that fractions are common.

The vertical (up and down) columns in the Periodic Table are called

• groups

• towers

• periods

• atomic numbers

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The Modern Periodic Table of Elements is arranged by

• atomic mass
• atomic number
• valence electrons
• number of isotopes