Chemistry Final Exam Review

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Questions and Answers

Consider MgF2 and answer the following questions: Is it ionic or covalent? How do you know?

Ionic (correct)

Covalent

Consider MgF2 and answer the following questions: What is the systematic name for this compound?

Magnesium fluoride

Consider MgF2 and answer the following questions: What charges are present on these ions?

Mg2+ and F-

Consider MgF2 and answer the following questions: Is it soluble in water?

True Signup and view all the answers

Consider MgF2 and answer the following questions: Write the electronic configuration for Mg and for F.

Mg: 1s²2s²2p⁶3s² F: 1s²2s²2p⁵ Signup and view all the answers

How many grams of H2O are formed by complete conversion of 32.00 g O2 with excess H2 according to the following equation: 2 H2 + O2 → 2 H2O

36.00 g Signup and view all the answers

Which molecule contains a triple bond? Draw each Lewis structure to confirm.

N2 Signup and view all the answers

Write total and net ionic equation for the following reaction. Identify the spectator ions. 3CaCl2 (aq) + 2 K3PO4 (aq) → Ca3(PO4)2 (s) + 6 KCl (aq)

Total ionic equation: 3Ca²⁺(aq) + 6Cl⁻(aq) + 6K⁺(aq) + 2PO₄³⁻(aq) → Ca₃(PO₄)₂(s) + 6K⁺(aq) + 6Cl⁻(aq) Net ionic equation: 3Ca²⁺(aq) + 2PO₄³⁻(aq) → Ca₃(PO₄)₂(s) Spectator ions: K⁺(aq) and Cl⁻(aq) Signup and view all the answers

When you run a reaction in a lab, you use a calorimeter to determine that 216 kJ of heat is absorbed. Pick the correct statement below.

the reaction is endothermic; ∆H = +216 kJ Signup and view all the answers

What would ∆H° (in kJ) be for the production of 75.00 g of Al2O3(s)? 4A1 (s) + 3O2 (g) → 2Al2O3 (s) ΔΗ° = -3351 kJ

-1256 kJ Signup and view all the answers

If 7.30 g of HCl and 4.00 g of NH3 are mixed, how many grams of NH4Cl can be formed? [MM: HCl = 36.5 g/mol; NH3 = 17.0 g/mol; NH4Cl = 53.5 g/mol] HCl(g) + NH3(g) → NH4Cl(s) How much remains of the excess reactant?

5.50 g of NH4Cl can be formed and 0.91 g of HCl remains. Signup and view all the answers

What are the stoichiometric coefficients needed to balance the following reaction? CH4 + O2 → CO2 + H2O

1 CH4 + 2 O2 → 1 CO2 + 2 H2O Signup and view all the answers

What is the oxidation number for phosphorus in H3PO4?

+5 Signup and view all the answers

Choose the correct 4 quantum numbers for the unpaired electron of aluminum. Write why the others might be incorrect (i.e., doesn't follow the rules of assigning quantum numbers, correspond to a different electron, etc.) a. n = 3, 1 = 0, ml = +2, ms = + 1/2 b. n = 1, 1 = 5, ml = -1, ms = + 2 c. n = 2, 1 = 0, ml = 0, ms = 1 d. n = 3, 1=1, ml =+1, ms = + ½ e. n = 2, 1=1, ml =+1, ms = 1

n = 3, 1=1, ml =+1, ms = + ½ Signup and view all the answers

Based on the reaction below, which statement is false? N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔΗ = - 46.11 kJ a. The reaction as written is endothermic. b. For the reverse reaction, ΔΗ° =+46.11 kJ c. 1 mole nitrogen reacts with 3 moles hydrogen to form 2 moles ammonia. d. The reaction as written is exothermic. e. This is the thermochemical equation for the formation of ammonia.

The reaction as written is endothermic. Signup and view all the answers

Which of the following is an example of a chemical change?

Broiling a steak on a grill Signup and view all the answers

Which of the following statements is correct about covalently bound atoms? Fix the statements that are incorrect. a. 2 electrons cannot be shared unequally between two atoms. b. 4 electrons can be shared equally between the two atoms. c. It is an electrostatic attraction between two oppositely charged ions. d. The electrons avoid a space called the overlap region of two orbitals. e. A covalent bond occurs when one electron is completely transferred from one atom to another.

4 electrons can be shared equally between the two atoms. Signup and view all the answers

Convert the following: 5.7x105 µg = ? mg?

570 mg Signup and view all the answers

Which ionic formula is incorrect? Fix it. a. NaCO3 b. KNO2 c. Sr(CN)2 d. (NH4)2SO4 e. NH4Cl

NaCO3 Signup and view all the answers

How many σ and π bonds are in the following: a. Single bond b. Double bond c. Triple bond

Single bond: 1 σ bond Double bond: 1 σ bond and 1 π bond Triple bond: 1 σ bond and 2 π bonds Signup and view all the answers

If you have 2.7 grams of KBr [MM = 119 g/mol], how many mL of water are needed to make a 3.6 M solution?

66 mL Signup and view all the answers

Consider the following reaction: Fe (s) + Cu2+ (aq) → Fe2+ (aq) + Cu (s). Which species in this reaction is being oxidized and which species is being reduced? a. Cu = oxidized; Fe = reduced b. Cu2+ = oxidized; Fe2+ = reduced c. Fe = oxidized; Cu2+ = reduced d. Cu2+ = oxidized; Cu = reduced e. None, this is not a redox reaction.

Fe = oxidized; Cu2+ = reduced Signup and view all the answers

Consider P2S5 and answer the following questions: Write the electron configuration for P and S.

P: 1s²2s²2p⁶3s²3p³ S: 1s²2s²2p⁶3s²3p⁴ Signup and view all the answers

Consider P2S5 and answer the following questions: Draw the orbital energy diagram for the valence electrons for P and S (in the shell n = 3).

P: 3s² 3px¹ 3py¹ 3pz¹ S: 3s² 3px² 3py¹ 3pz¹ Signup and view all the answers

What is the electron domain geometry and molecular geometry for NH3? Draw both the 3D shape and the Lewis structure. What is the hybridization of the orbitals around the central atom? How many lone pairs of electrons will you find on the central atom?

Electron domain geometry: Tetrahedral Molecular geometry: Trigonal pyramidal Hybridization: sp³ Number of lone pairs: 1 Signup and view all the answers

Predict the products for the following, remembering to balance the equation and write the appropriate phases: BaCl2 (aq) + K2SO4 (aq) → ?

BaCl2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KCl (aq) Signup and view all the answers

The value of ∆H° for the following reaction is -72 kJ. How many kJ of heat will be evolved when 3.0 g of HBr is formed in this reaction? H2(g) + Br2(g) → 2HBr(g)

-18 kJ Signup and view all the answers

A neutral molecule has the general form AX2E. What is the orbital hybridization (sp, sp², or sp³) of A?

sp² Signup and view all the answers

Study Notes

Exam Review

This review is a summary for the final exam.
The provided information on Canvas, the VSEPR Table, and the Periodic Table will be used on the final exam.
Review previous exams, recitation packets, exam review packets, quizzes for comprehensive preparation.

Problem 1

MgF2 : Determine if ionic or covalent. Provide reasoning.
Find the systematic name.
Identify ion charges.
Determine solubility in water.
Write electronic configurations for Mg and F.

Problem 2

Calculate grams of H₂O formed from complete conversion of 32.00 g O₂ with excess H₂.

Problem 3

Identify the molecule with a triple bond from options (F₂, Cl₂, O₂, I₂, N₂).
Draw Lewis structures to confirm.

Problem 4

Write total and net ionic equations for the reaction 3CaCl₂ (aq) + 2K₃PO₄ (aq) → Ca₃(PO₄)₂ (s) + 6KCl (aq).
Identify spectator ions.

Problem 5

Given 216 kJ of heat absorbed during a reaction in a lab using a calorimeter, choose the correct statement:
- Exothermic, ΔH = +216 kJ
- Endothermic, ΔH = -216 kJ
- Exothermic, ΔH = -216 kJ
- Endothermic, ΔH = +216 kJ
- Reaction will not run due to heat requirement

Problem 6

Calculate ΔH° (in kJ) for the production of 75.00 g of Al₂O₃(s). 4Al (s) + 3O₂ (g) → 2Al₂O₃ (s) ΔH° = -3351 kJ

Problem 7

Calculate the grams of NH₄Cl formed when 7.30 g HCl and 4.00 g NH₃ are mixed.
Determine the amount of the excess reactant.

Problem 8

Balance the following reaction: CH₄ + O₂ → CO₂ + H₂O.
Find the stoichiometric coefficients.

Problem 9

Calculate the oxidation number of phosphorus in H₃PO₄.

Problem 10

Determine the correct four quantum numbers for the unpaired electron in aluminum.
Explain why other options are incorrect.

Problem 11

Identify the false statement about the given reaction: N₂ (g) + 3H₂ (g) → 2NH₃ (g) ΔH = -46.11 kJ.
Reaction direction based on enthalpy change.

Problem 12

Identify the chemical change from a list of physical and chemical changes

Problem 13

Correct statements about covalently bonded atoms.

Problem 14

Convert 5.7 x 10⁵ µg to mg.

Problem 15

Identify and correct the incorrect ionic formula from a list.

Problem 16

Count σ and π bonds in different types of chemical bonds (single, double, triple).

Problem 17

Calculate mL of water needed to make a 3.6 M solution from 2.7 grams of KBr.

Problem 18

Determine which species is oxidized and reduced in the reaction Fe (s) + Cu²⁺ (aq) → Fe²⁺ (aq) + Cu (s).

Problem 19

Analyze P₂S₅ (phosphorus pentasulfide)
- Classify as ionic or covalent.
- Provide the systematic name.
- Write the electron configuration for P and S.
- Draw the orbital energy diagram for valence electrons in the n = 3 shell.

Problem 20

Determine the electron domain geometry and molecular geometry for NH₃.
Draw the Lewis structure.
Determine orbital hybridization.
Calculate lone pairs of electrons.

Problem 21

Predict products in the reaction BaCl₂ (aq) + K₂SO₄ (aq) →?
- Balanced equation with appropriate phases.

Problem 22

Given ΔH° = -72 kJ for H₂(g) + Br₂(g) → 2HBr (g), calculate the heat evolved when 3.0 g of HBr is formed.

Problem 23

Determine the orbital hybridization for a neutral molecule with general form AX₂E.

Problem 24

If photon A has a longer wavelength than photon B, which property of photon A is greater/lesser than that of photon B?

Problem 25

Calculate the volume a 2.5g sample of CO₂ occupies at 293 K and 0.984 atm.

Problem 26

Calculate grams of NaCl in 500 mL of 0.40 M NaCl.

Problem 27

Calculate the frequency of EM radiation with a wavelength of 530 mm.

Problem 28

Determine which molecules cannot participate in hydrogen bonding and explain why.

Problem 29

Calculate the new volume of a 1200 mL helium gas sample at 350 mmHg and 300 K, if pressure increases to 700 mmHg and temperature increases to 400 K.

Problem 30

Identify correct statements regarding Lewis structures.

Problem 31

Write the formation reaction of CH₃CH₂OH (1).

Problem 32

Calculate the number of hydrogen atoms in a 0.500 g sample of methane (CH₄).

Problem 33

Identify an atom based on electron configuration (1s² 2s² 2p⁶ 3s² 3p⁵).
Draw the Lewis dot symbol for this atom.
Determine the number of protons, neutrons, and electrons.
Write the complete atomic symbol.

Problem 34

Identify the nonpolar molecule from a list (CHF₃, NF₃, BF₃ , H₂O, HCN).
Draw VSEPR structures and show dipole arrows.

Problem 35

Write the full and noble gas electron configurations for calcium.

Problem 36

Analyze the compound PCl₅
- Write the full electron configurations for P and Cl
- Write the noble gas configurations for P and Cl
- Calculate the number of electrons needed for a full octet for P and Cl.
- State bonding type (transfer or share) between P and Cl.
- Classify the bond as ionic or covalent.
- Name the compound.
- Draw the Lewis structure
- Calculate formal charges (for P and one Cl atom).
- Determine the electron domain and molecular geometry.
- Determine the ideal bond angles.
- Determine if the molecule is polar or nonpolar

Problem 37

Analyze acetylene (C₂H₂)
- State bonding type (ionic or covalent)
- Draw the Lewis structure
- Determine orbital hybridization for each carbon. Explain how you know.
- Label sigma and pi bonds in the molecule.
- Calculate the energy and frequency of a photon with a wavelength of 750 nm.

Problem 38

Analyze the reaction of cadmium sulfate and potassium sulfide solutions.
- Write the complete balanced reaction, including phases.
- Write the total ionic equation.
- Identify spectator ions (if any).
- Write the net ionic equation.
- Calculate the moles of CdSO₄ in 750.0 mL of 0.850 M CdSO₄.

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Prepare for your Chemistry final exam with this comprehensive review. The quiz covers key topics such as ionic and covalent compounds, stoichiometry, and chemical reactions. Utilize the provided resources and previous materials for a thorough understanding and practice.