Chemical Bonding Questions and Answers

2. Decide whether the following statements are true (T) or false (F): (6 pts) (a) Colligative properties depend on the number of molecules present, not on the kind of molecules used. (b) Under identical conditions, the vapor pressure of a solution is expected to be higher than that of the pure solvent from which it is made. (c) Adding a nonvolatile solute to a pure solvent will decrease its freezing point. (d) Adding a nonvolatile solute to a pure solvent will increase its vapor pressure. (e) Adding a nonvolatile solute to a pure solvent will increase its boiling point. (f) Osmotic pressure is not a colligative property and has no dependence on solute concentration.

Give the complete electron configuration of rubidium (Rb). Put the number/letter orbital designation in the first box and the electrons in the superscript box. So, helium would have 1s in the first box and 2 in its superscript box. • How many total electrons does rubidium have? (add the superscripts to check) Give the noble gas shorthand electron configuration for Rb. [ ]

How would you explain the difference between -ide, -ate, and -ite endings? For example, how are nitride, nitrate, and nitrite different?

Complete the Lewis structures of the atoms and ions by adding electrons as needed. Li Select Draw Rings More 3 Na+ ||||||| S Li Erase Na Select Draw F // 3 Ć

Balance the following chemical reaction (Notice that a number one was included when no coefficient should appear.) Li₂ CrO4 + MnBr₂ ⇒ LiBr + MnCrO4 1,1,1,1 2,1,2,1 2,1,1,2 2,3,1,2 1,1,2,1

A flame test could be used to distinguish which of the following two substances most easily? Select one: arsenic acid and lead nitrate lithium nitrate and strontium nitrate potassium nitrate and calcium nitrate barium nitrate and manganese nitrate

Classify each substance based on the intermolecular forces present in that substance. Hydrogen bonding, dipole-dipole, and dispersion CO₂ HCI Dipole-dipole and dispersion only CO Answer Bank Dispersion only

c) The Balmer series are the results of excited electron at higher level relaxing to the electronic level of principle quantum number of n=2. Determine the excited electronic level, n, of this electron. 410.2 nm

Stoichiometry is best defined as the O qualitative relationship between reactants and products in a chemical reaction. study of chemical reactions. quantitative relationship between reactants and products in a chemical reaction. Given the reaction, how many moles of Z will be produced from 1.10 mol A, assuming excess B? 2A +3B4Y+5Z moles of Z= mol

Match the following terms to the correct definitions Column A 1. 2. 3. 4. 5. 6. 7. - - — products reactants covalent bond electronegativity ionic bond polar covalent bond valence electrons Column B a. a value that describes the relative strength with which an atom of an element attracts electrons to itself in a chemical bond. b. a force that holds oppoitely charged atoms (or groups of atoms) together c. the substances before a chemical reaction occurs d. a force that holds atoms together by unequally shared electrons e. a force that holds atoms together by sharing electrons f. the substances after a chemical reaction occurs g. the electrons in the outermost orbitals of an atom

For the each element, convert the given mole amount to grams. How many grams are in 0.0264 mol of lithium? mass: How many grams are in 0.350 mol of nickel? mass: How many grams are in 0.890 mol of neon? mass: g 60

5. Identify which of these Lewis structures (A, B, C or D) is correct for NOF and what is the VSEPR shape of the compound? (3 points for the structure and 3 for the shape. 6 points total) NOF A :: B :N::O:N::O: : F: :N C NOF: No: Lewis structure is VSEPR shape is

The formation of aluminum chloride can be described by the balanced chemical equation. 2 Al + 3 Cl₂ -> → 2 AICI 3 How many moles of Cl₂ molecules are required to react with 1.58 mol Al atoms? moles of Cl₂ required: mol Cl₂

Click the "draw structure" button to launch the drawing utility. The structure below contains a charged carbon atom. Add all hydrogen atoms and lone pair(s) to the structure below. Be sure to include the charge in your structure. In this problem only, it's ok to have a red box around the charged carbon atom in your structure.

What is the strongest intermolecular force present in 1-propanol? OH 1-propanol Multiple Choice Dipole-dipole Induced dipole-induced dipole Hydrogen bonding lon-ion

5:22 Which of the following compounds can form intermolecular hydrogen bonds with a molecule similar to itself? Multiple Choice O III IV || 11 III N H IV

When chlorine gains an electron to become a chloride ion with a -1 charge, it ends up with the noble gas electron configuration of argon. Why doesn't it become an argon atom?

F. copper (Cu) and oxygen (O₂) (4 pt.) balanced equation reaction type a G. potassium iodide solution (KI) and lead nitrate (Pb(NO3)2) solution (6 pt.) balanced equation b. total ionic equation reaction type net ionic equation Extra Credit: Balance the following equations. CaSiO3 (s) + C₂N2 (g) HF(g) -> H₂O (1) SiF4 (g) + H₂C₂O4 (aq) + CaF2 (s) + NH3 (g) 10 H₂O (1)

Step 2: Show the conversions required to solve this problem and calculate the grams of Al2O3. 38.8 g Al x grams of Al₂O3: 26.98 g Al 1 mole 0₂ Answer Bank 1 mole Al 1 mole Al₂O3 3 moles 0₂ 4 moles Al X 32.00 g 0₂ 101.96 g Al₂O3 2 moles Al₂O3 = g Al₂O3 g Al₂O3

Based on your knowledge of families select all the characteristics you would expect Argon to have: Ohighly reactive Ononreactive Ogas at room temperature liquid at room temperature odorless lustrous

14 Which of the following statements about resonance structures is not true? Multiple Choice Resonance structures are in equilibrium with each other. Resonance structures are not isomers. There is no movement of electrons from one form to another. Resonance structures differ only in the arrangement of electrons.

Which of the following is the appropriate conversion of (CH3)2CHOCH2CH2CH2OH to a skeletal structure? torin tor OH Multiple Choice ||| IV I 11 H III H IV OH

Refer to Q#5: Draw the Lewis structure for difluoromethane (CH₂F₂). As modeled and discussed in the live session: How many electrons is Carbon contributing to the CH₂F2 molecule? 04 0 1 06 08

2. Complete the table for the structure of each molecule and determine what the shape of each molecule is (3 Marks each, 9 Marks Total) [T] (UPLOAD IS REQUIRED) Molecular Compound SO4²- BrF5 SF4 Lewis Structure (show work) 9 poin VSEPR Shape Polarity

Refer to Q#2: Draw the Lewis structure for silicon dioxide. As modeled and discussed in the live session: What type of bonds are around the the central atom? O2 double bonds O4 single bonds O1 triple bond and 1 single bond

i. Draw the expected molecular shape, determine whether it is polar, and indicate the overall direction of the dipole moment. (You do NOT need to show resonance or formal charges AND if there are more than one isomer, please pick one for your answer. We will grade the following based on the isomer that you choose) ii. List all its symmetry elements and show all unique symmetry elements that are not the identity operator or an improper rotation. iii. Determine its point group. a. POCI3 b. POCIBr2 C. POCIBrl

13. Which of the following represents the molecular geometry of boron trifluouride, BF3, and nitrogen trifluoride, NF3, predicted by VSEPR theory? both structures are trigonal planar both structures are trigonal pyramidal BF3 is trigonal pyramidal and NF3 is trigonal planar BF3 is trigonal planar and NF3 is trigonal pyramidal 1 poir

8. Practice: In the spaces below, write and illustrate electron configurations for the next four elements: nitrogen, oxygen, fluorine, and neon. When you are finished, use the Gizmo to check your work. Correct any improper configurations. Nitrogen configuration: Oxygen configuration: Fluorine configuration: Neon configuration: 2s 15 25 1s 25 - 1s 2s 1s 2p 2p 2p 2p

Complete the following: a. Determine the number of valence electrons in NH₂OH b. Draw the corresponding Lewis structure and determine the molecular geometry c. Determine the number of o bonds d. Determine the number of π bonds e. Determine the hybridization of the central atom

▼ Part A HF 8. 0 8 8 8 8 8 Watch the animation and select the interactions that can be explained by hydrogen bonding. Check all that apply. ▸ View Available Hint(s) OCH4 molecules interact more closely in the liquid than in the gas phase. Ice, H₂O, has a solid structure with alternating H-O interactions. OH₂ Te has a higher boiling point than H₂S. OHF is a weak acid neutralized by NaOH. HF has a higher boiling point than HCl.

The octet rule states that atoms in molecules share electrons in such a way that each atom has a full valence shell. Determine whether each structure has the correct number of electrons and obeys the octet rule. Classify structures that have the correct number of electrons and obey the octet rule as valid, and those that do not as invalid. HH Ö H-C H H-H invalid structure valid structure :F: H- H valid structure invalid structure N valid structure invalid structure H H invalid structure valid structure

What intermolecular forces are present in each of the substances? Drag each item to the appropriate bin. ► View Available Hint(s) Dispersion forces only C₂H6 HCHO C6H14 C₂H5OH Dispersion forces and dipole-dipole forces H₂O Reset Help Dispersion forces, dipole-dipole forces, and hydrogen bonding

Write the full electron configuration for a neutral fluorine atom. full electron configuration: Draw the Lewis dot symbol for a neutral fluroine atom. Select Draw Rings More FL Erase Identify the subshells in the full electron configuration whose electrons are included in the Lewis dot symbol for the neutral fluorine atom. 1s 3s 2s 2p 3p

Predict whether each of the following bonds is ionic, polar covalent, or nonpolar covalent. Drag the appropriate items to their respective bins. lonic bond Mg-0 K-Br Si-O S-F Polar covalent bond Te-Br N-P Nonpolar covalent bond

V CaCl2 O Hydrogen bond Olonic bond Dispersion force Covalent bond Dipole-dipole attraction Submit HBr Part B Request Answer O Hydrogen bond Olonic bond O Dispersion force O Covalent bond Dipole-dipole attraction Submit Request Answer

Use the Lewis structure to determine the shape for each of the following molecules or polyatomic ions: Se03- Trigonal pyramidal Trigonal planar Bent (<120°) Tetrahedral O Linear Bent (<109.5°) Submit Part D 2- SO3²- Request Answe O Linear O Trigonal planar O Bent (<120°) O Tetrahedral O Trigonal pyramidal Bent (<109.5°) Submit Request Answer

Y C-Cor C-0 O C-C OC-O O the same polarity Submit Request Answer Part B P-Cl or P- Br OP-Cl OP-Br O the same polarity Submit Request Answer

O Cl Drag the appropriate labels to their respective targets. Cl Reset Help

Complete the following sentences about electronegativity. Match the words in the left column to the appropriate blanks in the sentences on the right. Make sure that each sentence is complete before submitting your answer. View Available Hint(s) carbon iodine positive smaller Reset Help 1. Electronegativity values increase from left to right across a period in the periodic table because there is an increase in the negative charge of the nuclei in this direction. 2. These values also increase from the bottom to the top of a group because the size of the atom decreases, resulting in a larger distance between the nucleus and the valence electron shell, which increases the attraction between the protons and electrons. 3. When considering both carbon and oxygen, oxygen is more electronegative because it appears further to the right in the same period of the periodic table. 4. When considering chlorine and iodine, chlorine is more electronegative because it appears higher in the same group of the periodic table.

The activation energy of an uncatalyzed reaction is 85 kJ/mol. The addition of a catalyst lowers the activation energy to 56 kJ/mol. ▼ Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 31 °C? Express the ratio to two significant digits. ke/ku= = VAEO Review I Constants I Periodic Table ?

Predict the shape for each molecule. Drag the appropriate items to their respective bins. Linear Bent (109) SF3+ Bent (120) PO, CIO I NO₂ Trigonal planar Trigonal pyramidal Tetrahedral Reset Help

Choose the shape that matches each of the following descriptions. Drag the appropriate items to their respective bins. Linear a molecule with a central atom that has four electron groups and two bonded atoms Bent (109) a molecule with a central atom that has two electron groups and two bonded atoms Bent (120) a molecule with a central atom that has three electron groups and two bonded atoms Trigonal planar Trigonal pyramidal Reset Help Tetrahedral

H3O+ Draw the molecule by placing atoms on the canvas and connecting them with bonds. Include all lone pairs of electrons. Place the charge of the polyatomic ion on the central atom in the correct structure. Brackets are not needed for this drawing.

12 of 33 Draw the correct Lewis structure for SF3 where the positive charge is attributed to the sulfur atom. Draw the molecule by placing atoms on the canvas and connecting them with bonds. Place the ion's charge on the center atom in the correct structure. Include all lone pairs of electrons. Brackets are not needed for this answer.

CCL4 Linear Trigonal planar Bent (109°) Tetrahedral Trigonal pyramidal Bent (120°) Request Answer

What is the molarity of CaCl, when 1.92 mol of CaCl, is dissolved in water to form 515 mL of solution? Select the correct answer below: O 3.73 M O 0.268 M O 3.73 x 10-3 M O 0.989 M

HCO₂ (with C as the central atom) Draw all the molecules by placing atoms on the grid and connecting them with bonds. Include all hydrogen atoms and all lone pairs of electrons. Show the charge of the ion over the central atom (C). A double-headed arrow or brackets are not needed.

Which attractive force is the weakest force between molecules? dipole-dipole attractions hydrogen bond dispersion force covalent bond

Total number of valence electrons in wing. Express your answer as an integer.

Write the symbols for the ions, and the correct formula for the ionic compound formed by each of the following: a. potassium and sulfur b. sodium and nitrogen d. gallium and oxygen c. aluminum and iodine