Electron Configuration & Periodic Trends

Standard Electron Configuration

100

What is the standard electron configuration for Li?

1s²2s¹

200

What is the standard electron configuration for Si?

1s²2s²2p⁶3s²3p²

300

Identify the element.

1s²2s²2p⁶3s²3p⁶4s²3d⁷

Co, cobalt

400

Identify the element:

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴

Se, Selenium

500

What is the standard electron configuration for the element in group 15, period 4?

As

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³

Orbital Notation

100

When drawing the orbital notation for an element, how many lines are drawn to represent the p-orbital?

3

200

Draw the orbital diagram for oxygen.

1s²2s²2p⁴

300

Using the noble gas shorthand, draw the orbital diagram for Ti.

[Ar]4s²3d²

400

The orbital diagram for which element in period 6 has only one arrow on each line of the p-orbital?

Bi

500

The orbital diagram for which element in period 5 has only 1 arrow in the s-orbital?

Rb

Noble Gas Notation

100

Write the noble gas notation electron configuration for S.

[Ne]3s²3p⁴

200

Write the noble gas notation electron configuration for Ni.

[Ar]4s²3d⁸

300

Identify the element:

[Kr]5s²4d¹⁰5p¹

In, Indium

400

Write the noble gas notation electron configuration for At.

[Xe]6s²4f¹⁴5d¹⁰6p5

500

Write the noble gas notation electron configuration for Uranium, U

[Rn]7s²5f⁴

Periodic Trends

100

Which element has a larger atomic radius: Al or Ca?

Ca

200

Which element has a larger ionization energy: S or Ge?

S

300

Which element has a larger electron affinity: Rb or P?

P

400

True or false and explain why:

Na has a larger radius and larger ionization energy than P.

False.  

Na does have a larger radius than P, but has a smaller ionization energy.  Radius and ionization energy are inversely related.

500

Which element has a larger electronegativity: Cl or Ar?

Cl

Ar is an exception because it is a noble gas

More Periodic Trends

100

Put the following elements in order of increasing radius: P, K, F, Ga

F < P < Ga < K

200

Put the following elements in order of increasing ionization energy: Mg, C, Cs, N

Cs < Mg < C < N

300

Put the following elements in order of increasing electron affinity: Sn, Se, As, Pb

Pb < Sn < As < Se

400

Put the following in order of increasing electronegativity: Br, Te, F, Se

Te < Se < Br < F

500

Put the following in order of increasing radius: 

Br^1-, Kr, Rb¹⁺

Rb¹⁺ < Kr < Br^1-

They all have 36 protons in nucleus, but Rb¹⁺ has the fewest electrons and therefore the electrons are pulled closer to the nucleus. Likewise, Br^1- has the most electrons, so they are not pulled as close to the nucleus.