Chemical Bonding Questions and Answers

What is the formula for nickel(III) oxide? Express your answer as a chemical formula.

Which statement is NOT true about the conditions for a reaction to occur? The collision must provide energy The higher the reactant concentration, the less likely the reaction will occur The reactants must collide All of the answers are true Reactants must align properly

Write the balanced dissociation equation for solid copper(I) hydroxide in aqueous solution. If it does not dissociate, simply write only NR.

Write the balanced NET ionic equation for the reaction when aqueous (NH4)3PO4 and aqueous Zn(NO3)2 are mixed in solution to form solid Zn3(PO4)2 and aqueous NH4NO3.

What information do we need to write the formula for the compound? (Select all that apply.) name of the compound atomic number of each element charge on the anion periodic table charge on the cation

Which of the following group 17 elements has the LARGEST monatomic ions? Why? Choose one: F-, because its neutral atom has the smallest atomic radius of the group. F-, because its neutral atom has the largest atomic radius of the group. Cl-, because its neutral atom has the smallest atomic radius of the group. Cl-, because its neutral atom has the largest atomic radius of the group. Br-, because its neutral atom has the smallest atomic radius of the group. Br-, because its neutral atom has the largest atomic radius of the group. I-, because its neutral atom has the smallest atomic radius of the group. I-, because its neutral atom has the largest atomic radius of the group.

How many grams of AlCl3 can be produced from the reaction that occurs between 94 g Al and 197 g of Cl₂? __ Al + _ Cl₂ -> __ AICI 3 Make sure to show all work (including the balanced chemical equation), identify the limiting reactant, and determine the amount of product that can be produced.

Which type of conclusion allows readers imagine their own conclusion? Open ended Personal Comment Mystery

Group 1 metals tend to lose one electron and become ions when in contact with nonmetal atoms. Which group of nonmetals will readily react with a Group 1 metal to form a compound in a one-to-one ratio (i.e., one metal atom combines with one nonmetal atom and both atoms are now stable)? Group 15 Group 16 Group 17 Group 18

The first four ionization energies of element M are approximately 744, 1492, 7.9x10^3, and 1.2×10^4 kJ/mol. What is the formula of the compound that this element forms when it bonds with oxygen (i.e. what is its oxide)? Include in your answer which periodic group does this element belong to.

What element forms an ion with an electronic configuration of 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 (or [Kr]) and a -2 charge? Give the symbol for the element. element symbol:

Use the orbital-filling diagram to show the electron configuration of helium, He. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all targets will be filled.

13. Acid catalyzed dehydration-condensation reactions of carboxylic acids and alcohols produce chemicals called esters. i. Using carbon skeletal notation, write the dehydration-condensation reaction that occurs between ethanol and butanoic acid. ii. What is the name of this ester?

The primary role of the protein keratin is to A) speed up the formation of nails and hair. B) provide strength to nails and hair. C) make curly hair curly. D) tell the body to store sugar.

Draw the Lewis structure for sulfur tetrafluoride, SF4, and then draw the electron pair geometry. What's the name of the molecular shape of sulfur tetrafluoride? Note: You can draw this on paper, take a picture, and paste the picture in your document.

Which of the following ranks bonds from lowest energy to highest energy? A) Triple bond between carbons < single bond between carbons < double bond between carbons B) Single bond between carbons < double bond between carbons < triple bond between carbons C) Single bond between carbons < triple bond between carbons < double bond between carbons D) Double bond between carbons < single bond between carbons < triple bond between carbons

Aqueous lead (II) nitrate, Pb(NO3)2 undergoes a double displacement reaction with aqueous sodium chloride, NaCl, in which a precipitate forms. If the precipitate contains lead, write the balanced chemical equation for this reaction. Be sure to include the states of each of the reactants and products.

The reactivity of an atom arises from the energy difference between the s and p orbitals. the existence of unpaired electrons in the valence shell. the average distance of the outermost electron shell from the nucleus. the potential energy of the valence shell. the sum of the potential energies of all the electron shells.

Which of the following is correct? During N2+ formation, one electron is removed from the bonding molecular orbitals During O2+ formation, one electron is removed from the antibonding molecular orbitals. During O2- formation, one electron is added to the bonding molecular orbitals. During N2- formation, one electron is added to the bonding molecular orbitals.

Calculate the percent composition by mass of C3H7NO. Fill in the blanks, answering in standard notation (not scientific notation) to the nearest tenth. A/ % C A % O A % H A % N

Which of the following is the balanced net ionic equation for the reaction between aqueous sodium hydroxide and aqueous iron (III) sulfate? NaOH(aq) + Fe2(SO4)3(aq) → Na2SO4(aq) + Fe(OH)3(s) O2 Fe3+6 OH → 2 Fe(OH)3(s) (aq) (aq) 2- + O 6 Na (aq) + 6 OH(aq) +2 Fe³+3 SO4(aq) →6 Natag) + 3 SO4 (aq) + 2 Fe(OH)3(s) O 6 NaOH(aq) + Fe2(SO4)3(aq) →3 Na2SO4(aq) + 2 Fe(OH)3(s)

Which of the following statements about chemical reactions is TRUE? Structurally, products are always less complex than reactants. O Dissolving a solid into water is an example of a chemical reaction. O Matter is rearranged in a chemical reaction. Chemical reactions do not depend on environmental conditions.

The ionization energy of an atom is a measure of its ability to attract and retain electrons the energy required to gain a valence electron the energy required to remove a valence electron its ability to remove inner electrons

Correctly balance the following redox reaction equation: Fe+3+ Sn+2 → Fe+2 + Sn+4 Oa) Fe+3+ Sn+2 → Fe+2+ Sn+4 Ob) 2 2 Fe+3+ Sn+2 → Fe+2 + 2 Sni Sn+4 Oc) 2 Fe+3+ Sn+2 → 2 Fe+2 + Sn+4 d) Fe+3+2 Sn+2 → Fe+2+2 Sn+4

Compare the F-CI-F angles in CIF₂+ and CIF₂. Using Lewis structures, determine the approximate bond angle in each ion. Think about which ion has the greater angle and why. CIF₂+, 120°; CIF2, 109.5° CIF₂+, 109.5°; CIF₂, 180° CIF2, 109.5°; CIF₂+, 180° CIF₂+, 109.5°; CIF₂, 90°

To determine the trends in basicity, sometimes the "availability" of the electrons in the base, to make the bond with the proton, is used. Explain this trend in basicity i.e why are the electrons in amide ion more "available" than the electrons in hydroxide ion, etc. NH₂-> HO- > CH3COO- > Cl-

Consider these structures for the formate ion, HCO₂-. Designate which two are resonance structures and which is equivalent to one of the resonance structures.

What is true about metals? Choose all that apply. Metals lose electrons to become cations Metals gain electrons to become anions Metal atoms form ionic bonds with other metals atom of the same element Metals conduct electricity Metal atoms form covalent bonds with other metal atoms of the same element Metals are brittle Metals are malleable

write the correct Lewis structures and assign a formal charge for each atom in N3-.

An element's most stable ion forms an ionic compound with bromine, having the formula XBr3. If the ion of element X has a mass number of 225 and has 86 electrons, what is the identity of the element, and how many neutrons does it have?

SO₂ can react with OH-, forming HSO3-. In this reaction, the SO2 acts as a Brønsted acid, accepting a proton from the OH-ion. the SO2 acts as a Lewis acid, accepting a proton from the OH-ion. the OH-ion acts as a Brønsted base, donating a proton to the SO2 molecule. the OH-ion acts as a Lewis acid, accepting an electron pair from the SO2 molecule to form a coordinate covalent bond. the OH-ion acts as a Lewis base, donating an electron pair to the SO2 molecule to form a coordinate covalent bond.

Which statement best predicts and explains the product of a single displacement reaction when the cation (A) with an oxidation number of +2 and an anion (B) with the oxidation number of -3 react and form a compound? A3B2 is the predicted formula with an overall charge of the compound being zero and each atom has 8 valence electrons in their outermost electron shell. OA+2B-3 is the predicted formula when each metal cation has a charge of +2 and each non metal has a charge of -3. B2A3 is the final formula for the metal anion bonding to the non-metal cation in a 2:3 ratio. A3B2 is the predicted formula is made when each metal cation gains three electrons from the anion while each nonmetal loses 2 electrons to each of the cations.

ammonium carbonate see results Place a small amount of ammonium carbonate in a test tube. Attach a piece of rubber tubing to the test tube and gently heat the tube. Bubble the gases produced through a saturated calcium hydroxide solution and then through a phenolphthalein indicator solution. The solid formed when the products of the reaction are passed through the calcium hydroxide solution is calcium carbonate. Phenolphthalein is an acid-base indicator that is bright pink or purple in a basic solution. 1. Complete and balance the reaction. 2. Classify the reaction.

The reason for water having such a high boiling point is the presence of Van Der Waals Forces London Dispersion Forces Unknown Forces Hydrogen bonds

1) Draw Lewis structures for the following OXYACIDS acids. For each, MAKE SURE... i) You provide the total valence electron count. ii) EVERY bond is shown. iii) iv) NOTE: EVERY lone pair is shown ALL formal charges are shown, ON the atom they belong on (no brackets) On the quiz, you will be asked for some of these, and we probably will NOT cover all of them in class. Furthermore, you will NOT get a periodic table - so start memorizing the valence electron counts for H, Li, Na, K, B, C, N, O, S, F, Cl, Br, and I. a) Nitric acid (_______ total electrons) c) Sulfuric acid (total electrons) b) Acetic acid (_______total electrons) d) Perchloric acid (_______ total electrons)

What kind of intermolecular forces act between a dichlorine monoxide molecule and a hydrogen cyanide (HCN) molecule?

Specify the hybridization at the atoms labelled a-d. For each atom enter one of the following: sp3, dsp2, sp2, sp3d, or sp. Hybridizations are normally written with superscripted numbers, but OWL expects no to this question.

A chemical engineering student is testing out various liquids in her lab. She has seven substances: Substance A: C6H14 (hexane). It is non-polar, mixing well with oil but not with water. Substance B: H₂O2 (hydrogen peroxide). It contains two O-H bonds, and does not mix with oil or hexane. Substance D: CH3CONH2 (acetamide). It has two N-H bonds. Substance E: CH3COOH (acetic acid). It mixes well with water, has an O-H bond, and is polar. Substance F: (CH3)2CO (acetone). There are no O-H bonds, though it is polar. Substance G: C₂H4(NH2)2 (ethylendiamine). Multiple N-H bonds, and mixes well with some polar substances. Substance C: C₂H5OH (ethanol). Ethanol mixes well with water and hydrogen peroxide. She needs a substance that will mix well with silanol, SiH3OH, shown below. For safety reasons, she knows it cannot contain nitrogen and it must be able to do hydrogen bonding with other substances. Which substances are okay to use, according to this information?

When 3.00 g of sulfur are combined with 3.00 g of oxygen, 6.00 g of sulfur dioxide (SO₂) are formed. What mass of oxygen would be required to convert 7.00 g of sulfur into sulfur trioxide (SO3)?

Which of the following Periodic Table trends (characteristics) is incorrect? electronegativity decreases left to right across the periodic table atomic radii decreases left to right across the periodic table ionization energy decreases from top to bottom on the periodic table electron affinity decreases from top to bottom on the periodic table

When a magnesium atom becomes a cation, the size of the radius ... increases because it gained electrons increases because it lost electrons decreases because it lost electrons decreases because it gained electrons

Despite the fact that atomic radius generally increases down a group, the Pd-Cl distance in PdCl42- is essentially identical to the Pt-Cl distance in PtCl42. Which is the best explanation of why the two bond lengths are the same? PdCl42- is tetrahedral, while PtCl42- is square planar, and so shorter bonds are expected. The presence of the 14 lanthanides between Pd and Pt makes Pt unexpectedly small The large negative charge on the complex ions makes the chloride-chloride repulsions, not the metal-chloride attractions, the dominant factor in determining the bond distance The Pd-Cl bond is largely ionic, whereas the Pt-Cl is largely covalent, and so the atoms necessarily have to be closer together to form a covalent bond The metal-chlorine bonds are highly covalent and are insensitive to the trend in atomic radius

Which statement(s) describing the structure and bonding in nitromethane (H3CNO₂) is(are) false? Each of the three bonds to nitrogen is a different length and the nitrogen atom has a trigonal planar geometry are both false statements. Each of the three bonds to nitrogen is a different length. None of these statements are false that is, the three statements are all true. The molecule exhibits resonance. The nitrogen atom has a trigonal planar geometry.

Rank the enthalpies of fusion, sublimation and vaporization for water. A) Sublimation = vaporization = fusion B) Vaporization < sublimation < fusion C) Fusion < sublimation <vaporization D) Fusion <vaporization < sublimation E) Cannot be determined.

Which statement(s) correctly describe(s) the carbonate ion (CO32-)? I. All three carbon-oxygen bond distances are the same. II. All three bond angles are 120°. III. It will combine with an acid to make CO₂ and H₂O. A) I only B) II only C) I and II only D) I and III only E) I, II and III

In the gas phase PCl, exists as individual molecules but in the solid it takes on the ionic structure PC14 PC16. What are the geometries of these three species? A) All three structures are trigonal bipyramidal. B) PCl5 is trigonal bipyramidal, PCl4 is see-saw shaped, and PCI 6- is octahedral. C) PCl5 is trigonal bipyramidal, PCl4+ is tetrahedral, and PCl6- is octahedral. D) PCl5 is trigonal bipyramidal, PCl4+ is square planar, and PCl6- is a distorted octahedral shape. E) PCl5 is square bipyramidal, PCl4+ is see-saw shaped, and PCI6- is square planar.

What is the approximate bond angle in AsCl3? 180 90 120 109

Use bond energies to estimate the enthalpy change (AH) for the following reaction: N₂H4 (g) + 2 F₂ (g) → N₂ (g) + 4 HF (g) Enter your calculated answer below and be sure to upload your work and calculations to receive full credit. The work submitted should include list of bonds broken and bonds formed and calculated energy for each. (Note: Correct answers without supporting work earn 0 points)

Draw the Lewis and VSEPR structure for CO2. A. Give the electron geometry. B. Give the bond angle. C. Give the molecular geometry D. Does it have polar covalent bonds or nonpolar covalent bonds? E. Is the molecule polar or nonpolar? F. List all the intermolecular forces present. G. Give the strongest intermolecular force present.

Three inequivalent resonance structures for the cyanate ion, OCN", are shown below. Assign formal charges to all atoms in the resonance structures and identify the more likely resonance structure. Note: If a row is not needed, leave it blank.