Question: If 5.12 g of oxygen gas

> Although the valence electron pairs in ammonia have a tetrahedral arrangement, the overall geometric structure of the ammonia molecule is not described as being tetrahedral. Explain.

> Suppose that 1.28 g of neon gas and 2.49 g of argon gas are confined in a 9.87-L container at 27 °C. What would be the pressure in the container?

> If a gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in an evacuated 1.04-L container at 25 °C, what will be the partial pressure of each gas and the total pressure in the container?

> What general principles determine the molecular structure (shape) of a molecule?

> We often collect small samples of gases in the laboratory by bubbling the gas into a bottle or flask containing water. Explain why the gas becomes saturated with water vapor and how we must take the presence of water vapor into account when calculating t

> Determine the partial pressure of each gas as shown in this figure. Note: The relative numbers of each type of gas are depicted in the figure. 1.00 atm о Не Ne Ar

> Explain why the measured properties of a mixture of gases depend only on the total number of moles of particles, not on the identity of the individual gas particles. How is this observation summarized as a law?

> What mass of neon gas would be required to fill a 3.00-L flask to a pressure of 925 mm Hg at 26 °C? What mass of argon gas would be required to fill a similar flask to the same pressure at the same temperature?

> What evidence do we have that the solid form of water is less dense than the liquid form of water at its freezing/melting point?

> A tank contains a mixture of 52.5 g of oxygen gas and 65.1 g of carbon dioxide gas at 27 °C. The total pressure in the tank is 9.21 atm. Calculate the partial pressure (in atm) of each gas in the mixture.

> Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. c

> Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. c

> Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. c

> Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. s

> Consider Fig. 14.10. Imagine you are talking to a friend who has not taken any science courses, and explain how the figure demonstrates the concept of vapor pressure and enables it to be measured. From figure 14.10 Diethyl ather vapor -Vacuum -H;O v

> What do we mean by a dynamic equilibrium? Describe how the development of a vapor pressure above a liquid represents such an equilibrium.

> In carbon compounds a given group of atoms can often be arranged in more than one way. This means that more than one structure may be possible for the same atoms. For example, both the molecules diethyl ether and 1-butanol have the same number of each ty

> Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. C2H6 b. NF3 c. C4H10 d. SiCl4

> Write a Lewis structure for each of the following simple molecules. Show all bonding valence electrons pairs as lines and all nonbonding valence electron pairs as dots. a. H2S b. SiF4 c. C2H4 d. C3H8

> Compare and contrast the bonding found in the H2 (g) and HF(g) molecules with that found in NaF(s).

> Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. NBr3 b. HF c. CBr4 d. C2H2

> Give the total number of valence electrons in each of the following molecules. a. B2O3 b. CO2 c. C2H6O d. NO2

> Give the total number of valence electrons in each of the following molecules. a. N2O b. B2H6 c. C3H8 d. NCl3

> If you’ve ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed con

> What mass of helium gas is needed to pressurize a 100.0-L tank to 255 atm at 25 °C? What mass of oxygen gas would be needed to pressurize a similar tank to the same specifications?

> Given each of the following sets of values for an ideal gas, calculate the unknown quantity. a. P = 782 mm Hg; V =? n = 0.210 mol; T = 27 °C b. P =? mm Hg; V = 644 mL; n = 0.0921 mol; T = 303 K c. P = 745 mm Hg; V = 11.2 L; n = 0.401 mol; T =? K

> Show how Charles’s gas law can be derived from the ideal gas law.

> Show how Boyle’s gas law can be derived from the ideal gas law.

> What do we mean by an ideal gas?

> Explain what the “duet” and “octet” rules are and how they are used to describe the arrangement of electrons in a molecule.

> Consider a sample of ice being heated from -5 °C to +5 °C. Describe on both a macroscopic and a microscopic basis what happens to the ice as the temperature reaches 0 °C.

> Given the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 782.4 mm Hg; V = ?; n = 0.1021 mol; T = 26.2 °C b. P = ? mm Hg; V = 27.5 mL; n = 0.007812 mol; T = 16.6 °C c. P = 1.045 atm; V = 45.2 mL; n = 0.00

> For each of the following pairs, indicate which is larger. a. I or F b. F or F- c. Na+ or F-

> For each of the following pairs, indicate which is smaller. a. Fe or Fe3+ b. Cl or Cl- c. Al3+ or Na+

> For each of the following pairs, indicate which species is larger. Explain your reasoning in terms of the electron structure of each species. a. Mg2+ or Mg b. Ca2+ or K+ c. Rb+ or Br- d. Se2- or Se

> For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species. a. H or H- b. N or N3- c. Al or Al3+ d. F or Cl

> When dry ammonia gas (NH3) is bubbled into a 125-mL sample of water, the volume of the sample (initially, at least) decreases slightly. Suggest a reason for this.

> Ionic solids are generally considerably harder than most molecular solids. Explain.

> Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?

> How do ionic solids differ in structure from molecular solids? What are the fundamental particles in each? Give two examples of each type of solid and indicate the individual particles that make up the solids in each of your examples.

> On the basis of the smaller units that make up the crystals, cite three types of crystalline solids. For each type of crystalline solid, give an example of a substance that forms that type of solid.

> Describe a simple mercury barometer. How is such a barometer used to measure the pressure of the atmosphere?

> Why are the dipole–dipole interactions between polar molecules not important in the vapor phase?

> What mass of neon gas is required to fill a 5.00-L container to a pressure of 1.02 atm at 25 °C?

> If two gases that do not react with each other are placed in the same container, they will completely with each other.

> If 2.71 g of argon gas occupies a volume of 4.21 L, what volume will 1.29 moles of argon occupy under the same conditions?

> If 3.25 moles of argon gas occupies a volume of 100. L at a particular temperature and pressure, what volume does 14.15 moles of argon occupy under the same conditions?

> On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other. a. aluminum and bromine b. aluminum and oxygen c. aluminum and phosphorus

> If 0.00901 mole of neon gas at a particular temperature and pressure occupies a volume of 242 mL, what volume would 0.00703 mole of neon occupy under the same conditions?

> If a 0.475-L sample of neon gas is heated from 27 °C to 82 °C at constant pressure, what will be the volume of the sample at the higher temperature?

> If a gaseous mixture is made of 3.50 g of He and 5.75 g of Ar in an evacuated 2.05-L container at 25 °C, what will be the partial pressure of Ar in the container?

> An expandable vessel contains 729 mL of gas at 22 °C. What volume will the gas sample in the vessel have if it is placed in a boiling water bath (100. °C)?

> A sample of a gas at 0.780 atm occupies a volume of 0.501 L. If the temperature remains constant, what will be the new pressure if the volume increases to 0.794 L?

> If the pressure on a 2.10 * 104 mL sample of gas is doubled at constant temperature, what will be the new volume of the gas?

> Convert the following pressures into mm Hg. a. 0.903 atm b. 2.1240 * 106 Pa c. 445 kPa d. 342 torr

> If 0.214 mole of argon gas occupies a volume of 652 mL at a particular temperature and pressure, what volume would 0.375 mole of argon occupy under the same conditions?

> If 10.0 g of liquid helium at 1.7 K is completely vaporized, what volume does the helium occupy at STP?

> On the basis of their electron configurations, predict the formula of the simple binary ionic compounds likely to form when the following pairs of elements react with each other. a. aluminum, Al, and sulfur, S b. radium, Ra, and oxygen, O c. calcium,

> At what temperature does 4.00 g of helium gas have a pressure of 1.00 atm in a 22.4-L vessel?

> Suppose two separate 100.0-L tanks are to be filled, one with helium and one with hydrogen. What mass of each gas is needed to produce a pressure of 2.70 atm in its respective tank at 24 °C?

> What is the pressure inside a 10.0-L flask containing 14.2 g of N2 at 26 °C?

> You have 1 mole of an ideal gas in a balloon. How must the volume change so that the pressure in the balloon doubles and the temperature in °C is halved (assume the temperature is a positive value)? a. The volume must decrease by more than half the orig

> Carbon dioxide gas, in the dry state, may be produced by heating calcium carbonate. CaCO3(s) / CaO(s) + CO2(g) What volume of CO2, collected dry at 55 °C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of CaCO3?

> The formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure. Formula Compound Name Molecular Structure CO, NH3 SO3 H,0 ClO,-

> Which of the following compounds or ions exhibit resonance? a. O3 b. CNO- c. AsI3 d. CO32- e. AsF3

> Write electron configurations for the most stable ion formed by each of the following elements. Do not use the noble gas notation. Write out the complete electron configuration. Electron Configuration of the Most Stable lon Element Na K Li Cs

> For a mixture of gases in the same container, the total pressure exerted by the mixture of gases is the of the pressures that those gases would exert if they were alone in the container under the same conditions.

> List the bonds P-Cl, P-F, O-F, and Si-F from least polar to most polar.

> For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain the same. a. V = 9.14 L at 24 °C; V =? at 48 °C b. V = 24.9 mL at –12 °C; V = 49.9

> Compare the electronegativities of each pair of atoms. State the element of each pair that has the greater electronegativity. Symbol for Element with Greater Electronegativity Pair P and CI Ca and N N and As

> Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar covalent. a. H2 b. K3P c. NaI d. SO2 e. HF f. CCl4 g. CF4 h. K2S

> When doing any calculation involving gas samples, we must express the temperature in terms of the temperature scale.

> What is the expected ground-state electron configuration for the element with one unpaired 5p electron that forms a covalent compound with fluorine?

> Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds. a. CO32- b. HNO3 (hydrogen is bonded to oxygen) c. NO2- d. C2H2

> Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds. a. SO2 b. SO3 c. HCO3- (hydrogen is bonded to oxygen) d. HCN

> For each of the following molecules, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. a. Cl2O b. CCl4 c. BeCl2 d. BCl3

> Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. a. chlorate ion b. chlorite ion c. perchlorate ion

> Using the VSEPR theory, predict the molecular structure of each of the following molecules. a. Cl2O b. OF2 c. SiCl4

> For the indicated atom in each of the following molecules, give the number and the arrangement of the electron pairs around that atom. a. C in CCl4 b. Ge in GeH4 c. B in BF3

> For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the mass of gas remain constant. a. V = 25.0 L at 0 °C; V = 50.0 L at? °C b. V = 247 mL at 25 °C; V = 255 mL at? °C c. V = 1.00 mL

> Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s) + O2(g) SO2(g) 2SO2(g) + O2(g) 2SO3(g) What volume of O2(g) at 350. °C and a pressure of 5.25 atm is nee

> Chemicals placed in a microwave oven and exposed to microwave radiation can increase in temperature if they possess a net dipole moment. Which of the following molecules can get hot in an operating microwave oven? CCl4, H2O, HCl, BH3, CO2

> Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit resonance, draw the various possible resonance forms.

> Select which of the following ions has the Lewis structure: a. B22- b. C22- c. N22- d. O22- e. F22- [:X-X:12-

> Consider the following reaction: Zn(s)+ 2HCl(aq) ZnCl2(aq) + H2(g) What mass of zinc metal should be taken so as to produce 125 mL of H2 measured at STP when reacted with excess hydrochloric acid?

> Welders commonly use an apparatus that contains a tank of acetylene (C2H2) gas and a tank of oxygen gas. When burned in pure oxygen, acetylene generates a large amount of heat. 2C2H2(g) + 5O2(g) / 2H2O(g) + 4CO2(g) What volume of carbon dioxide gas at ST

> Write the Lewis structure for each of the following atoms. a. He (Z = 2) b. Br (Z = 35) c. Sr (Z = 38) d. Ne (Z = 10) e. I (Z = 53) f. Ra (Z = 88)

> For each of the following pairs, indicate which is smaller. a. Rb+ or Na+ b. Mg2+ or Al3+ c. F- or I- d. Na+ or K+

> Which noble gas has the same electron configuration as each of the ions in the following compounds? a. calcium bromide, CaBr2 b. aluminum selenide, Al2Se3 c. strontium oxide, SrO d. potassium sulfide, K2S

> A widely used weather instrument called a barometer can be built from a long, thin tube of glass that is sealed at one end. The tube is completely filled with mercury and then inverted into a small pool of mercury. The level of the mercury inside the tub

> For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the mass of gas remain constant. a. V = 2.01 * 102 L at 1150 °C; V = 5.00 L at ? °C b. V = 44.2 mL at 298 K; V = ? at 0 K c. V = 44

> What simple ion does each of the following elements most commonly form? a. sodium b. iodine c. potassium d. calcium e. sulfur f. magnesium g. aluminum h. nitrogen

> Which of the following contains a metal ion that does not have a noble gas electron configuration? AgCl, BaCl2, TiO2, ScF3, KNO3

> For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. N-Cl b. N-P c. N-S d. N-C

> The electrons involved in a C-F bond could be considered a. closer to C because carbon has a larger radius and thus exerts greater control over the shared electrons. b. closer to F because fluorine has a higher electronegativity than carbon. c. closer

> Consider the following unbalanced chemical equation for the combination reaction of sodium metal and chlorine gas: Na(s) + Cl2(g) / NaCl(s) What volume of chlorine gas, measured at STP, is necessary for the complete reaction of 4.81 g of sodium metal?

> Which of the following molecules contain polar covalent bonds? a. carbon monoxide, CO b. chlorine, Cl2 c. iodine monochloride, ICl d. phosphorus, P4

> On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. a. H-O b. O-O c. H-H d. H-Cl

> For each of the following pairs of elements, identify which element would be expected to be more electronegative. It should not be necessary to look at a table of actual electronegativity values. a. Be or Ba b. N or P c. F or Cl

> A(n) chemical bond represents the equal sharing of a pair of electrons between two nuclei.