chapter 6 and 7 review (periodic trends and electron configuration)

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

Tags

NGSS.HS-PS1-2

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 

Tags

NGSS.HS-PS1-1

Which atom has the largest atomic radius?

• barium

• strontium

• radium

• calcium

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

• +1

• +7

• -7

• -1

• 17

Tags

NGSS.HS-PS1-1

The energy necessary to excite an electron from n=5 to n=6 is the _______ the energy necessary to excite an electron from n=4 to n=5.

• greater than

• less than

• equal to

What is this element?
[Xe] 6s²4f¹⁴5d⁹

• Mercury
• Gold
• Platinum
• Thallium

Tags

NGSS.HS-PS1-1

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

• Gallium

• Aluminum

• Magnesium

• Strontium

Which of the following will have a lower ionization energy than iron (Fe)?

• Helium (He)

• Copper (Cu)

• Calcium (Ca)

• Magnesium (Mg)

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

Tags

NGSS.HS-PS1-1

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.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2