Periodic 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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The element with the largest electronegativity in the halogens is - 

• At
• F
• Cl
• Br

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The element with the lowest electronegativity in Period 3 is -

• Na

• Cl

• Ar

• Mg

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The electronegativity of Cl is the highest in Period 3. Why?

• Cl is the largest and has the greatest effective nuclear charge

• Cl is the smallest and has the lowest effective nuclear charge

• Cl is the largest and has the lowest effective nuclear charge

• Cl is the smallest and has the greatest effective nuclear charge

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A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

• chemical reactivity

• atomic radius

• energy levels

• orbit

As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more mass.
• the atoms have less mass
• the atoms have more protons.
• the atoms have less electrons.

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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

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Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

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Which of the following will have a larger radius than Zinc?

• Gallium

• Aluminum

• Magnesium

• Strontium

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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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