Which of the following statements are CORRECT? Ionic bonds form when one or more valence electrons are transferred from one atom to another. Covalent bonds involve sharing of electrons between atoms. Ionic bond formation is always exothermic, covalent bond formation is always endothermic. 1 and 2 1,2 , and 3 3 only 1 only 2 only
For an atom of a main group element, the number of valence electrons is equal to its group number. the principle quantum number of its oster shellit. its number of core clectrons. its period number. eight minus its group number.
Which of the following compounds is expected to have the strongest ionic bonds? NaF NaI RbF CsI CsBr
Arrange in order of electronegativity (1 = highest and 5 = lowest): Sr, Al, Cl, P, Cs 1 [Choose] 2 [Choose] 3 Choose [ 4 [Choose] 5 [Choose]
Use VSEPR theory to predict the molecular geometry of H3O+. bent trigonal-planar trigonal-pyramidal linear T-shaped
The central atom in XeF4 is surrounded by 4 single bonds, no double bonds, and no lone pairs of electrons. 4 single bonds, no double bonds, and 2 lone pairs of electrons. 2 single bonds, 2 double bonds, and no lone pairs of electrons. 3 single bonds, 1 double bond, and no lone pairs of electrons. 3 single bonds, 1 double bond, and 1 lone pair of electrons.
Use VSEPR theory to predict the molecular geometry of IF5. sec-saw octahedral tetrahedral square-pyramidal trigonal-bipyramidal
Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of the nitrite ion, NO2-: The electron-pair geometry is linear, the molecular geometry is linear. The electron-pair geometry is tetrahedral, the molecular geometry is linear. The electron-pair geometry is tetrahedral, the molecular geometry is bent. The electron-pair geometry is trigonal-planar, the molecular geometry is linear. The electron-pair geometry is trigonal-planar, the molecular geometry is bent.
What is the hybridization of the carbon atom in carbon disulfide? CS2 sp2 sp3 sp3d2 sp sp3d
Which of the following is the correct molecular geometry for ozone. O3? tetrahedral linear trigonal bipyramidal square planar trigonal planar, bent
What is the molecular geometry around a central atom that is sp2 hybridized, has three sigma bonds, and has one pi bond? tetrahedral trigonal-bipyramidal trigonal-planar trigonal-pyramidal linear
What is the molecular geometry around a central atom that is sp3 hybridized and has one lone electron-pair? trigonal-planar trigonal-pyramidal bent trigonal-bipyramidal linear
Which of the following characteristics apply to PCl3? 1. nonpolar molecule 2. polar bonds 3. trigonal-pyramidal molecular geometry 4. sp2 hybridized 3 and 4 1, 2, and 3 1, 2, 3, and 4 1 and 2 2 and 3
Sulfur trioxide is known to be planar with all the oxygen atoms equidistant from the central sulfur atom. On the basis of these facts, which of the following statements are CORRECT? 1. It can be represented by three equivalent resonance structures. 2. The sulfur atom is sp2 hybridized. The molecule is nonpolar. 1 only 1, 2, and 3 2 only 3 only 1 and 2
Which of the following elements is most likely to display sp3d hybridization? phosphorus oxygen nitrogen hydrogen carbon
What is the geometry of the orbital that is sp2 hybridized? octahedral trigonal pyramidal linear tetrahedral trigonal planar
According to the molecular orbital theory, which of the following molecules has a bond order of three? O2 F2 Be2 N2
According to molecular orbital theory, which of the following species is unlikely to exist? O2 He2 N2 H2 Cl2
Using only the periodic table, rank each set of main-group elements in order of decreasing atomic size and explain your answer: K, Ga, Ca
At 338 mm Hg and 72 ∘C, a sample of carbon monoxide gas occupies a volume of 0.225 L. The gas is transferred to a 1.50−L flask and the temperature is reduced to −15 ∘C. What is the pressure of the gas in the flask? 37.9 mm Hg 67.8 mm Hg 5.48 ′ 10 4 mm Hg 3.018 ′ 10 3 mm Hg 8.91 mm Hg
A 45.0 L gas cylinder contains 988 g He at 23 ∘C. What is the pressure inside the cylinder? (R = 0.08206 L×atm/mol×K) 133 atm 533 atm 10.4 atm 41.4 atm 101 atm
If a balloon at 25 ∘C and a volume of 500. mL is cooled to liquid nitrogen temperature (77 K), what will be its volume (in mL)? Assume that this is a constant-pressure process. mL
A mass of 2.703 g of an unknown gas is introduced into an evacuated 5.00 L flask. If the pressure in the flask is 0.914 atm at 78 ∘C, which of the following gases might be in the flask? NO NH3 C2H2 H Cl N2
An unknown hydrocarbon gas sample has a volume of 500.0 mL and a mass of 0.3569 g at STP. What is the molecular weight of the gas in units of g/mol?
The mass of 560 cm3 (at STP) of an unknown gas is 1.60 g. This gas could be chlorine (71 g/mol) oxygen (32 g/mol) sulfur dioxide (64 g/mol) hydrogen (2 g/mol) carbon dioxide (44 g/mol)
Which of the following masses of gases has the greatest volume at 300 ∘C and 1 atm? 50 g C3H8 (g) 50 g I2 (g) 50 g C6H6 (g) 50 g Br2 (g) All of these masses of gas occupy the same volume.
What volume is occupied by 35.0 g of C2H2 at 471 mm Hg and 21 ∘C? Show all calculations and report your answer to the correct number of sig figs. (R = 0.08206 L×atm/mol×K).
At constant temperature, 7.72 L of Cl2 at 458 mm Hg is compressed to 3.75 L. What is the final pressure of Cl2? Show all calculations and report your answer to the correct number of sig figs.
If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the smallest temperature change?
Which one of the following statements is INCORRECT? Increasing the thermal energy of a gas increases the motion of its atoms. Energy is the capacity to do work. Kinetic energy is the energy associated with motion. Exothermic processes transfer heat from the surrounding into the system. Energy is neither created nor destroyed in chemical reactions.
Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 3.30 10 2 J of heat per gram dissolved in water. In a coffee-cup calorimeter, 4.40 g NH4NO3 is dissolved in 100.0 g of water at 21.0 ∘C . What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/g⋅K. 3.3 ∘C 20.9 ∘C 17.7 ∘C 24.3 ∘C 20.2 ∘C
One statement of the first law of thermodynamics is that in any chemical process the heat flow must equal the change in enthalpy. the heat flow in or out of a system is independent of pathway. the total work done on a system must equal the heat absorbed by the system. the total energy flow in or out of a system is equal to the sum of the heat transferred to or from the system and the work done by or on the system. the amount of work done on a system is dependent of pathway.
Which of the following chemical equations does not correspond to a standard molar enthalpy of formation? C(s) 1/2 O2(g) CO(g) SO2(g) 1/2 O2(g) SO3(g) H2(g) 1/2 O2(g) H2O(l) N2(g) 2 O2(g) N2O4(g) Ca(s) C(s) 3/2 O2(g) CaCO3(s)
A chemical reaction in a bomb calorimeter evolves 5.17 kJ of heat. If the heat capacity of the calorimeter is 1.08 kJ/∘C, what is the temperature change of the calorimeter? 5.58 ∘C 0.209 ∘C 6.25 ∘C 4.09 ∘C 4.79 ∘C
Calculate DH for the following reaction, CaO(s) + CO2(g) CaCO3(s) given the thermochemical equations below. 2Ca(s) + O2(g) 2CaO(s) DH = −1270.2 kJ C(s) + O2(g) CO2(g) DH = −393.5 kJ 2Ca(s) + 2C(s) + 3O2(g) 2CaCO3(s) DH = −2413.8 kJ
When 27.0 g of an unknown metal at 88.4 ∘C is placed in 115 g H2O at 21.0 ∘C, the final temperature of the water is 23.7 ∘C. What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g⋅K 1.4 J/g⋅K 0.34 J/g⋅K 0.51 J/g⋅K 0.74 J/g⋅K 0.94 J/g⋅K
If 136 J is required to change the temperature of 8.75 g of nickel by 35.0 K, what is the specific heat capacity of nickel? Show all work and calculate to the correct number of sig figs.
Determine the heat of reaction for the oxidation of iron, 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) given the thermochemical equations below. 2 Fe(s) + 6 H2O(l) 2 Fe(OH)3(s) + 3 H2(g) DH = +321.8 kJ 2 H2O(l) 2 H2(g) + O2(g) DH = +571.7 kJ Fe2O3(s) + 3 H2O(l) 2 Fe(OH)3(s) DH = +288.6 kJ Show all work and calculate to the correct number of sig figs.
Write the net ionic equation for the reaction of aqueous sodium carbonate with aqueous iron(III) chloride.
Write the net ionic equation for the reaction of aqueous lead(II) nitrate with aqueous sodium bromide.
Write the net ionic equation for the reaction of aqueous lithium hydroxide and aqueous nitric acid.
What are the spectator ions in the reaction between aqueous perchloric acid and aqueous potassium hydroxide?
Write the balanced chemical equation for the following: Gaseous ammonia reacts with gaseous hydrogen chloride to form solid ammonium chloride. What is the coefficient in front of ammonium chloride? 1 2 5 4 3
What is the net ionic equation for the reaction of aqueous silver nitrate with aqueous potassium bromide?
Write the balanced chemical equation for the following: Acetylene gas (C2H2) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely blue flame. The products of the combustion of acetylene are carbon dioxide gas and water vapor. What is the coefficient in front of carbon dioxide?
Write a balanced chemical equation for the following (include s, l, g. aq and use an = for an arrow): Explosive decomposition of dynamite: liquid nitroglycerine (C3H5N3O9) explodes to produce a mixture of gases - carbon dioxide, water vapor, nitrogen, and oxygen.
Write the balanced chemical equation for the following: The destruction of a marble statuary by acid rain: aqueous nitric acid reacts with solid calcium carbonate to form gaseous carbon dioxide, liquid water and aqueous calcium nitrate. What is the coefficient in front of nitric acid?
Write the net ionic equation for the reaction of aqueous sodium hydroxide with aqueous iron(III) chloride.
Write the net ionic equation for the reaction of aqueous lithium hydrogen carbonate with aqueous hydrochloric acid.
Write the net ionic equation for the reaction of aqueous rubidium carbonate and aqueous calcium perchlorate?
Write the net ionic equation for the reaction of aqueous sodium hydroxide with aqueous iron(III) chloride.
What is the net ionic equation for the reaction of aqueous barium nitrate with aqueous sodium sulfate?
What are the spectator ions in the reaction between aqueous chloric acid and aqueous potassium sulfite?
Consider the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). Which ions are spectator ions?