CCU4 PES day 2

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Multiple Choice

Which peak represents electrons closest to the nucleus?

• A

• B

• C

• they are all equally close to the nucleus.

Multiple Choice

What element is represented?

• Lithium

• Carbon

• Neon

• Oxygen.

• Fluorine

Multiple Choice

Label the peaks in your packet
What element is represented?

• Boron

• Neon

• Argon

• Strontium

• Aluminum

Labelling

Label with the peaks

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3s²

3p⁶

2s²

2p⁶

1s²

Multiple Choice

 The diagram above represents two electrons with 

• a. opposite spins.
•  b. the same spin.
• c. different energies.
• d. different energy levels.

Multiple Choice

What is the electron configuration of Boron

• 1s² 2s³

• 1s² 2s² 2p¹
• 1s² 2s² 3s¹

Labelling

What is the orbital diagram for Boron?​

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Multiple Choice

Which of the following is the orbital notation for oxygen?

Multiple Choice

Which of the following is the orbital diagram for nitrogen?

Multiple Choice

What electron configuration matches an oxygen atom?

• 1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵
• 1s²2s²2p⁴
• 1s²2s²2p⁶
• 1s²2s²2p⁶3s²3p⁶4s²3d¹

Drag and Drop

What is the electron configuration of fluorine

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• What else do we know?

Multiple Choice

What is the final sublevel of Bromine's Electron Configuration

• 5s⁵

• 5p⁴

• 3p⁵

• 4p⁵

​1s²

Drag and Drop

What is the shorthand / noble gas electron configuration of Iodine

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[Kr]

[Xe]

Drag and Drop

What is the shorthand / noble gas electron configuration of Platinum

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[Xe]

[Rn]

Multiple Choice

How many electrons can the d sublevel hold?

• 8
• 10
• 2
• 4

Multiple Choice

Which is associated with more energy? 

• 2p
• 2s
• 3p
• 1s

Multiple Choice

What is the maximum number of electrons that an s orbital can have?

• 1 electron

• 2 electrons

• 3 electrons

• 4 electrons

Multiple Choice

What is the noble gas configuration for Sulfur?

• [Ar] 3p⁴
• [He] 3s² 3p⁴
• [Ne] 3s² 3p⁴
• [Na] 3s² 3p⁴
  

Multiple Choice

How many electrons can the p sublevel hold?

• 8
• 6

• 2
• 4

Multiple Choice

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

• Zinc (Zn)

• Copper (Cu)

• Nickel (Ni)

• Germanium (Ge)

Multiple Choice

In an electron configuration, what follows 4s?

• 4p

• 3d

• 4s

• 2f

Multiple Choice

Choose the Noble Gas that you would use to begin the shorthand configuration of the following element. Iron (Fe)

• [He]

• [Ne]

• [Ar]

• [Kr]

Multiple Choice

Carbonate

• Cr₂O₄^-2
• CH₃COO^-
• CO₃^-2
• CN^-

Multiple Choice

Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Multiple Choice

What is this element?
1s²2s²2p⁶3s²

• Neon
• Magnesium
• Aluminum
• Potassium

Multiple Choice

Write the electron configuration for the element.

• 1s¹2s¹2p³3s¹

• 1s²2s²2p⁵3s¹

• 1s2s2p3s

• 1s²2s²2p⁶3s¹

Multiple Choice

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

Multiple Choice

What is this element? 
1s²2s²2p⁶3s²3p⁶
4s²3d¹⁰4p⁶

• Argon
• Krypton
• Selenium
• Bromide

Multiple Choice

What atom matches this electron configuration?
1s²2s²2p⁶3s²

• Neon
• Magnesium
• Aluminum
• Potassium

Multiple Choice

Electron arrangement that uses arrows

• Electron configuration
• Shorthand configuration
• Lewis dot structure
• Orbital diagram

Multiple Choice

Which has the greater EN: 
N or C?

• C
• N

Multiple Choice

The PES spectrum below is for the element _______________.

• O

• Ne

• N

• F

Multiple Choice

Magnesium's ion

• Mg⁺
• Mg²⁺
• Mg^-
• Mg^2-

Multiple Choice

An orbital can at most hold how many electrons?

• 1 electron
• 2 electrons
• 3 electrons
• 4 electrons

Multiple Choice

Which is the largest atom?

• O

• B

• Be

• N

Multiple Choice

Which element is depicted from this atomic orbital diagram?

• Carbon
• Nitrogen
• Oxygen
• Phosphorus

Multiple Choice

HCO₃^1-

• carbonate

• bicarbonate

• chlorate

• perchlorate

Multiple Choice

What is the abbreviated electron configuration for barium?

• [Xe] 6s²
• [Rn] 6s²
• [Ar] 4s² 3d¹⁰ 4p⁵
• [He] 2s² 3p¹

Multiple Choice

What is this element? 
[Ar]4s²

• Calcium
• Sodium
• Scandium
• Titanium

Multiple Choice

PO₃^3-

• Phosphate

• Potassium

• Phosphite

• Permanganate

Multiple Choice

What is the shorthand configuration for Tin?

• [Xe]5s²4d¹⁰5p²

• [Xe]5s²4d¹⁰5p²

• [Kr]5p²

• [Kr]5s²4d¹⁰5p²

Multiple Choice

CN^1-

• hydroxide

• acetate

• cyanide

• permanganate

Multiple Choice

Which subshell is highlighted in the periodic table below?

• 5s

• 5p

• 4p

Multiple Choice

Nitrite

• NO₂^-
• NO₃^-
• MnO₄^-
• NH₄⁺

Multiple Choice

What is the proper Noble Gas notation for the electron configuration of a neutral atom of Germanium (Ge)?

• [Ne] 4s²3d¹⁰4p²

• [Ar] 4s²3d¹⁰4p²

• [Kr]4s²3d¹⁰4p²

Multiple Choice

Which orbitals are spherically symmetrical?

• s

• p

• d

• f

Multiple Choice

ClO₃^-

• Carbonate

• Chlorate

• Nitrate

• Chlorite

Multiple Choice

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

Multiple Choice

[Ne]3s¹ is the noble gas configuration for which element?

• sodium
• lithium
• fluorine
• aluminum

Multiple Choice

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