Preparation and Properties of Compounds Questions and Answers

What is the the shape (molecular geometry) of NO₂Cl?

What is the electron-pair geometry for S in SF5CI? C What is the the shape (molecular geometry) of SF5CI?

Use the following standard enthalpies of formation to estimate the N-H bond energy in ammonia: N(g), 472.7 kJ/mol; H(g), 216.0 kJ/mol; NH3(g). -46.1 kJ/mol.

Draw the Lewis structure for PCl5

Draw a Lewis diagram for CH3CN.

Draw all resonance structures for the acetate ion, CH3COO-

Draw the Lewis structure for BrF4-

A. An element with the valence electron configuration 3s² would form a monatomic ion with a charge of In order to form this ion, the element will ___ ____ electron(s) from/into the subshell(s). B. If an element with the valence configuration 4s23d7 loses 2 electron(s), these electron(s) would be removed from the subshell(s).

Draw the Lewis structure for POCl3 in the window below and then answer the questions that follow.

Determine the formal charge of CI in CIO3-. 0 -1 3 2 1 2

What is the electron-pair geometry for S in SF5CI? What is the the shape (molecular geometry) of SF5CI?

What is the electron-pair geometry for B in BH₂ What is the the shape (molecular geometry) of BH₂?

a. Predict the molecular structure and bond angles for SO₂. Approximate bond angles are sufficient. Molecular Structure = Bond Angles = b. Predict the molecular structure and bond angles for OCl₂. Approximate bond angles are sufficient. Molecular Structure = Bond Angles- =

Some plant fertilizer compounds are (NH4)2SO4, Ca3 (PO4)2, CaO, HBO3 and FeCl3. Which of these compounds contain both ionic and covalent bond. (NH4)2SO4 Cao FeCl3 H₂ BO3 Ca3(PO4)2

What is the formula of the ion? A monatomic ion with a charge of -2 has an electronic configuration of 1s²2s²2p 3s²3p64s²- This ion is a(n) What is the chemical symbol of the noble gas this ion is isoelectronic with?

Draw the Lewis structure for NO₂Cl in the window below and then answer the questions that follow.

A monatomic ion with a charge of +2 has an electronic configuration of 1s²2s²2p 3s²3p6. This ion is a(n) What is the chemical symbol of the noble gas this ion is isoelectronic with?

Arrange the following elements in order of increasing electronegativity: indium, tellurium, antimony, tin smallest largest

2. Use the balanced equation given to solve the following problems. Na3PO4 + 3 AgNO3 -> Ag3PO4 + 3 NaNO3 a. If you have 9.44 grams of Na3PO4, how many grams of AgNO3 will be needed for complete reaction?

For the following molecule, write the Lewis structure, predict the molecular structure (including bond angles), give the expected hybrid orbitals on the central atom and predict the overall polarity.

Choose the best action to correct this structure. Remove a bond between the two nitrogen atoms and use the electron pairs to form an additional lonepair on each nitrogen atom. Add another bond between the two nitrogen atoms. Add two additional bonds between the two nitrogen atoms. Add an additional lone pair to each nitrogen atom.

3. Use the balanced equation given to solve the following problems. All substances are in the gas phase. N2 (g) + 3 H₂ (g) ⇒ 2NH3(g) a. When 5.50 mol N₂ react, what volume of NH3, measured at STP, will be formed?

A. What is the hybridization of the central atom in IFs? Hybridization = What are the approximate bond angles in this substance ? Bond angles = B. What is the hybridization of the central atom in XeF₂? Hybridization = What are the approximate bond angles in this substance ? Bond angles =

The chemical reaction system that can be used to produce the biofuel methanol, CH3OH (g),is represented by the following equation: 2 H2(g) + CO (g) = CH3OH (g) K = 10.5 at 500 K Question #1) When the concentrations of hydrogen, H2 (g); carbon monoxide, CO (g); and methanol are 0.25 mol/L, 0.25 mol/L, and 0.040 mol/L, respectively, is the system at equilibrium? Place your answer in blank #1. Question #2) If not, predict the direction in which the equilibrium will shift and explain why. Place your answer in blank #2.

Chemical kinetics is the study of factors that affect the rate of a chemical reaction the chemical properties of substances the rate of a change in concentration the physical properties of substances none of the above

Indicate whether each of the following describes a gas, a liquid, or a solid. The substance has no definite volume or shape The particles in a substance do not interact with each other The particles in a substance are held in a rigid structure

Which of the following pairs of gas samples would have closest to the same number of particles? A. 73.1 g of SF6 and 1.0 g of H₂ B. 8.8 g of CO₂ and 10.4 g of C3H8 C. 10.8 g of Ne and 36.0 g of Kr D. 4.0 g of O₂ and 4.0 g of N₂

A 29.3-g sample of water at 300. K is mixed with 50.7 g water at 350. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.

When elements combine to form compounds: their properties are an average of all elements in the compound. their properties do not change. their properties are completely random. their properties change completely.

A sample of an ideal gas at 22.2 atm and 11.4 L is allowed to expand against a constant external pressure of 1.17 atm at a constant temperature. Calculate the work in units of kJ for the gas expansion. (Hint. Boyle's law applies.)

Calculate the root mean square velocity for the O₂ molecules in a sample of O₂ gas at 11.8°C. (R = 8.3145 J/K mol) 471 m/s 95.9 m/s 9.88x10^26 m/s O272 m/s 14.9 m/s

An unknown diatomic gas has a density of 3.164 g/L at STP. What is the identity of the gas?

Uranium hexafluoride is a solid at room temperature, but it boils at 56°C. Determine the density of uranium hexafluoride at 70.°C and 735 torr.

A mixture of 1.40 g H₂ and 1.30 g He is placed in a 1.00-L container at 23°C. Calculate the partial pressure of each gas and the total pressure. PH₂ PHe PTOTAL

The name of the 8th most abundant gas in dry air at sea level is

The name of the 7th most abundant gas in dry air at sea level is

A compound is found to contain 30.45 % nitrogen and 69.55 % oxygen by mass. The empirical formula for this compound is The molar mass for this compound is 46.01 g/mol. The molecular formula for this compound is

Calculate the percentage composition for XeO3. Mass percentage of xenon Mass percentage of oxygen

You carry out the synthesis of Ca(OH)2 using the 2.04 g of KOH and 3.02 g of CaCl2-2H₂O as in #1, and your yield of dry Ca(OH)2 is 1.22 g. What is the percent yield for the reaction?

You fill a balloon with 2.50 moles of gas at 27°C at a pressure of 1.92 atm. What is the volume of the balloon? 18.9 L 2.84 L 32.0 L 22.4 L 118 L

Which of the following statements is true for real gases? As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas. As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas.

Calculate the percent by mass of each element in the following compounds. HClO2

A scientist measures the standard enthalpy change for the following reaction to be -222.0 kJ: 2H₂O₂(I)→ 2H₂O(l) + O₂(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(I) is ___ kJ/mol.

A 162-mL sample of gas is collected over water at 22°C and 753 torr. What is the volume of the dry gas at STP? (The vapor pressure of water at 22°C = 20. torr) 142 mL 182 mL 149 mL 129 mL none of these

A binary compound of carbon and hydrogen has the following percentage composition: 79.89% carbon, 20.11% hydrogen by mass. If the molar mass of the compound is determined by experiment to be between 30 and 31 g/mol, what are the empirical and molecular formulas of the compound? Empirical formula: Molecular formula:

Use the thermochemical data that follow to calculate the value of AH° for the reaction: 4B -> 2A+ C +2F ΔH° = 60 kJ A + 2B → E ΔH° = -40 kJ C+2D -> 2E ΔH° = 45 kJ F + 2A -> D 55 kJ 170 kJ 70 kJ -170 KJ -65 KJ

A compound is found to contain 37.32 % phosphorus, 16.88 % nitrogen, and 45.79 % fluorine by mass. The empirical formula for this compound is The molar mass for this compound is 82.98 g/mol. The molecular formula for this compound is

Calculate the work for the expansion of CO₂ from 1.0 to 3.0 liters against a pressure of 1.0 atm at constant temperature. 0 L-atm -2.0 L atm 3.0 L atm 2.0 L atm -3.0 L atm

Choose the process that requires the most energy when the temperature of 23.4 g ice at -25.0 °C is raised to 37.0 °C. Warming the water Warming the ice to 0.0 °C Melting the ice All of the processes require essentially the same amount of energy.

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2BrF3(g)- →Br₂(g) + 3F₂(g)