Unit Test 4

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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NGSS.HS-PS1-1

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

 Which of the following generally applies to the noble gases? 

• high ionization energy, low electronegativity, high reactivity
• high ionization energy, high electronegativity, high reactivity
• low ionization energy, low electronegativity, low reactivity
• high ionization energy, low electronegativity, low reactivity 

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NGSS.HS-PS1-1

Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 

• Fluorine has less energy levels.
• Chlorine has more electrons in its outer shell
• Fluorine has more protons.
• None of these

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

What is ionization energy?

• Energy needed to destroy an atom
• Energy required to remove an electron
• Energy needed to split an electron
• Energy required to add an electron

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As you look down a group, ionization energy and electronegativity

• increases

• decreases

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Which element has the greater ionization energy?

• Magnesium (Mg)

• Phosphorus (P)

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Which element has the greater ionization energy?

• Iodine (I)

• Chlorine (Cl)

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List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr

• P, Co, Sr, Cs
• Cs, Sr, Co, P
• Sr, Cs, Co, P
• P, Co, Cs, Sr

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NGSS.HS-PS1-1

NGSS.HS-PS1-2