Honors Chemistry Midterm Review 23-24

Chemistry Basics/Electrons

100

Perform the following conversions:

70 mL to DL

845 kg to g

0.007 DL

845,000 g

200

Give the full electron configuration for Nickel and give the noble gas configuration for Vanadium.

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁸

[Ar] 4s²3d³

300

What is the Aufbau Principle, Pauli Exclusion Principle, and Hund's Rule?

Aufbau = Lowest energy orbitals fill first

Pauli = No two electrons can have the same four quantum numbers (must have opposite spins)

Hund's = Must put one electron in each orbital before doubling up

400

Which of the following is a chemical change? (More than one is correct)

Boiling point, flammability, evaporation, red color, neutralize an acid

Flammability and neutralize an acid

500

Lithium-6 is 4% abundant and lithium-7 is 96% abundant. What is the average mass of lithium?

6.96 g

Periodic Table

100

What property is based on the ability of an atom to attract electrons to itself within a compound?

Electronegativity

200

Arrange the following in order of increasing ionization energy: O, F, Si, P

Si, P, O, F

300

Arrange the following elements in order from highest electronegativity to lowest electronegativity: Sb, S, F, Se

F, S, Se, Sb

400

Arrange the following set of ions in order of increasing atomic radii: S^2-, Cl^-, P^3-

Cl^-, S^2-, P^3-

500

What is the trend for atomic size on the periodic table and WHY is this the trend?

Increases to the left and down a group. Increase down a group due to adding another orbital and decreases to the left due to adding another proton, causing a higher effective nuclear charge.

Bonding

100

Give the formulas for Silver sulfite and Triphosphorus nonafluoride

Give the names of Be(C₂H₃O₂)₂ and PbO₂

Ag₂SO₃ and P₃F₉

Beryllium acetate and Lead (IV) oxide

200

Draw the lewis structure for calcium bromide and the lewis structure for carbon dioxide.

[Ca]²⁺ [Br]^-₂

O=C=O

300

Determine if the following molecule is polar or nonpolar and list all of the IMFs present in the compound - H₂S

Polar - LDFs and Dipole-Dipole Forces

400

Draw the Lewis structure for XeF₄ and give the electronic geometry, molecular geometry, bond angles, and hybridization.

Octahedral, square planar, 90˚, sp³d²

500

Which of the following molecules will have the highest boiling point and why? CH₃OH or CH₃OCH₃

Draw the Lewis Structure for the compound that will have the highest boiling point

CH₃OH because of hydrogen bonding

Reactions

100

Determine the type of reaction below, predict the products, and balance the final equation:

C₆H₁₄ + O₂ -->

Combustion

2C₆H₁₄ + 19O₂ --> 12CO₂ + 14H₂O

200

Determine the type of reaction below, predict the products, and balance the final equation

Mg (s) + AlPO₄ (aq) →

Single Replacement

3Mg (s) + 2AlPO₄ (aq) → 2Al (s) + Mg₃(PO₄)₂ (aq)

300

Determine the type of reaction below, predict the products, and balance the final equation

FeBr₃ + H₂SO₄ --> 

Double Replacement

2FeBr₃ + 3H₂SO₄ --> Fe₂(SO₄)₃ + 6HBr

400

An aqueous solution of potassium iodide and silver nitrate are mixed. Give the overall, total ionic, and net ionic equations.

KI (aq) + AgNO₃ (aq) --> KNO₃ (aq) + AgI (s)

500

Aqueous solutions of sodium carbonate and manganese(V) chloride are mixed. Give the overall, total ionic, and net ionic equation.

5Na₂CO₃ (aq) + 2MnCl₅ (aq) --> Mn₂(CO₃)₅ (s) + 10NaCl (aq)

Random

100

What neutral element has 2 valence electrons in the 4s shell and 2 half filled p orbitals (in addition to its core electrons)?

Ge (Germanium)

200

How many valence electrons in an atom with the following electron configuration? 1s²2s²2p⁶3s²

What would be the highest energy subshell in the Nb³⁺ ion?

2 / 5s

300

What is the molar mass of Al₂(SO₃)₃?

294.17 g

400

Draw the Lewis structure for BrF₅ and give the electronic geometry, molecular geometry, bond angles, and hybridization.

Octahedral, Square pyramidal, 90, sp³d

500

How many grams are in 2.5 x 10¹⁹ molecules of trinitrogen dioxide? (Use proper sig figs)

3.1 x 10^-3 grams