Inorganic Chemistry Questions

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

For the elements Cs, F, and S, the order of increasing electronegativity is: Cs < F< S OS< F< Cs CS <S<F F<Cs < S None of these choices are correct.

Draw the Lewis structure for ICI4-

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.

The energy of a particular color of green light is 3.87×10^-22 kJ/photon. The wavelength of this light is

Use bond energies to predict ΔH for the following reaction: CH4 (9) + 4F2 (g) → CF4(g) + 4HF (g)

Draw the Lewis structure for PCl5

Draw all resonance structures for the nitric acid molecule, HNO3 (NO₂OH).

Draw a Lewis diagram for CH3CN.

Draw all resonance structures for the acetate ion, CH3COO-

What is the electron-pair geometry for P in PCl5 What is the the shape (molecular geometry) of PC5?

Draw the Lewis structure for BrF4-

(Do not use noble gas notation and enter the subshells in the order in which they are filled. Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s²2s¹.) a. Lit b. Tlt c. Br d. I

Draw a Lewis structure for NH4+.

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 a Lewis structure for C3H6-

Draw the Lewis structure for SF5CI in the window below and then answer the questions that follow.

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

Calculate the energy for the transition of an electron from the n=4 level to the n = 3 level of a hydrogen atom. ΔE= This is an _________ process.

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 formal charge on each atom in OBr-? A. = -1, Br=0 B. = -1, Br = +1 C. +1, Br = -2 D. O-2, Br = +1 E. = 0, Br = -1

What is the electron-pair geometry for N in NO₂Cl?

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- =

Write electron configurations for the most stable ion formed by each of the elements Al, Sr, O, and F Electron configuration for the most stable ion of Al = Electron configuration for the most stable ion of Sr = Electron configuration for the most stable ion of 0 = Electron configuration for the most stable ion of F =

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

A. What is the hybridization of the central atom in IF5? Hybridization = What are the approximate bond angles in this substance ? Bond angles = B. What is the hybridization of the central atom in SF4? Hybridization = What are the approximate bond angles in this substance ? Bond angles =

Use the octet rule to predict the formula of the compound that would form between arsenic and hydrogen, if the molecule contains only one arsenic atom and only single bonds are formed.

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?

Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements. a. C and Cl b. Cs and Br c. Na and Cl d. F and F e. Li and Cl f. K and F

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

For each of the following compounds, classify it with the atomic-scale picture that best represents it in solution or as insoluble in aqueous solution.

Compare the magnitude of the lattice energy for each of the following two ion pairs. (a) Cs+ and Br- separated by a distance of 393 pm (b) Cs+ and I- separated by a distance of 423 pm

Draw all resonance structures for the sulfur trioxide molecule, SO3.

A monatomic ion with a charge of +1 has an electronic configuration of 1s²2s²2p 3s²3p64s²3d¹04p6. This ion is a(n) What is the formula of the ion? What is the chemical symbol of the noble gas this ion is isoelectronic with?

A monatomic ion with a charge of -2 has an electronic configuration of 1s²2s²2p 3s²3p64s²3d¹04p6 This ion is a(n) What is the chemical symbol of the noble gas this ion is isoelectronic with?

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.

From 600 C.E. to 1450 C.E, trade networks increased the level of affluence in many societies, which had an adverse effect on A. children B. education C. the economy D. women

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.

Which of the following statements is true, according to the collision theory? all collisions result in reactions entities must collide to react entities that collide but are incorrectly oriented will form a different product all entities in a collision have the same quantity of kinetic energy none of the above

a. Give the expected hybridization of the central atom of XeF4. b. Give the expected hybridization of the central atom of SO3.

A. What is the hybridization of the central atom in XeF4? Hybridization = What are the approximate bond angles in this substance ? Bond angles = B. What is the hybridization of the central atom in IBr3? Hybridization = What are the approximate bond angles in this substance ? Bond angles =

A chemist conducted a study of the decomposition of phosphine gas, PH3 (g), into phosphorous gas, P4(g), and hydrogen gas. This reaction is represented by the following balanced chemical equation: 4 PH3(g) → P4(g) + 6 H2(g) She determined the rate of reaction with respect to the consumption of phosphine gas to be -0.0024 mol/(L s). What are the rates of formation of phosphorous gas and hydrogen gas in this experiment? Place your answer for phosphorous gas in the first blank and your answer for hydrogen gas in the second blank.

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?

Silver bromide was prepared by reacting 200.0 grams of magnesium bromide and an adequate amount of silver nitrate. Calculate the percent yield if 375.0 grams of silver bromide was obtained from the reaction.

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 =