Exam 2 Jeopardy Activity

Atomic Trends

100

What two directions do you have to go to increase Atomic Size on the periodic table?

Left of the Period and Down the Group

200

Rank the following elements according to Atomic size, in decreasing order: Cl, W, Cs, Sb 

Cs(biggest), W, Sb, Cl(smallest)

300

Using the given Electron affinity values, tell me which element is LEAST likely to form and anion

A) Cl (-359 kj/mol)

B) Be (+48 kj/mol)

C) Ca (-2 kj/mol)

Be, this is because a more negative value would be most likely to form an anion, while a more positive value is least likely to form an anion. 

400

Lattice energy is proportional and inversely proportional to what? (Think about the equation)

Proportional to the Charge of the Cation and Anion and inversely proportional to the distance between both ions (or Size)

500

Which as the lowest lattice energy: CsBr, NaCl, SrO, CaO, KBr (taken from the practice exam)

CsBr because it has the bigger cation and anion, which makes them relatively lower in energy because there are weaker electrostatic attractions 

Models of the Atom

100

An ionic bond is a _______ of electrons from one nonmetal and one metal. 

Transfer

200

What is the Partial electron configuration of Chloride

[Ne]3s²3p⁶

300

Is this the right configuration for chromium: 

[Ar]4s¹3d⁵

True or False, explain why it is that way. 

True, because the electron in the s orbital moving to the d orbital increases the stability of the atom in its ground state. Neutral atoms try their best to be as stable as possible. 

 

400

True or False: Nonpolar covalent bonds involve equal sharing on electrons and polar covalent bonds involve unequal sharing of electrons?

True 

500

What is the partial electron configuration of Iridium (Z=77)

[Xe]4f¹⁴5d⁷6s²

Configurations and Diagrams

100

Would a partial orbital diagram or a condensed electron configuration be used to best visualize the m_s of a specific electron in an orbital?

Partial orbital diagram, because you can use the arrows to show the direction each electron will be spinning, either +1/2 (up) or -1/2 (down)

200

What is the Condensed Electron Configuration of Copper 

[Ar]4s¹3d¹⁰

300

Draw the partial orbital diagram for Nitrogen

*can't draw on here...

400

Draw the Pseudo and inert electron configuration of Germanium (Ge). What are the charges resulted in both configurations? 

Pseduo - [Ar]3d¹⁰ results in +4 charge

Inert-pair - [Ar] 4s²3d¹⁰ results in +2 charge

500

How many Inner, outer, and valence electrons are there for Ag

46, 1, 1 

Lewis Structures

100

What electrons are used when we draw out Lewis Structures?

Valence Electrons 

200

How many Valence electrons are there in total of COCl₂

24 valence electrons in total

300

How many lone pair are present in the molecule NHCl₂?

7 in total. 3 on each chlorine atom and 1 on nitrogen 

400

Calculate the formal charge of all atoms present in CO₂. One oxygen in single bonded to central carbon, and the other oxygen is triple-bonded to central carbon. 

Single bond oxygen = -1

Central Carbon = 0

Triple bonded oxygen = +1

500

How many possible resonance structures are there for OCS and which structure contributes the most to the resonance hybrid?

3 possible structures. The structure that shows zero formal charges on all atoms (the one with 2 double bonds) contributes most to the resonance hybrid. 

Molecular Shape

100

What is the only possible Molecular Shape for a SN number of 2 

Linear

200

How many Bonding groups are there in CO₂

Just 2, lone pairs don't count as bonding groups, since the are the E part in the AXE configuration. 

300

What are the two possible bond angles for Trigonal Bipyrimidal

90 and 120 degrees

400

What is the SN number and Molecular Shape of AX₃E₂. Also give the bond angles of the bonded atoms?

SN=5 

Molecular shape: T-shaped

Bond angle: less than 90^o

500

Molecular shape of XeF₄

Square Planar 

AX₄E₂