The Components of Matter

The following charges on individual oil droplets were obtained during an experiment similar to Millikan's. Determine a charge for the electron( in coulombs), and explain your answer:
$\mathbf{-}\mathbf{1}\mathbf{.}\mathbf{602}\mathbf{\times }{\mathbf{10}}^{\mathbf{19}}\mathit{C}$ ; $\mathbf{-}\mathbf{4}\mathbf{.}\mathbf{806}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{C}$; $\mathbf{-}\mathbf{8}\mathbf{.}\mathbf{010}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{C}$; $\mathbf{-}\mathbf{14}\mathbf{.}\mathbf{42}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{C}$.

A compound of copper and sulfur contains 88.39 g of metal and 44.61 g of nonmetal. How many grams of copper are in5264 kg of the compound? How many grams of sulfur?

Fluorite, a mineral of calcium, is a compound of the metal with fluorine. Analysis shows that a 2.76-g sample of fluorite contains 1.42 g of calcium. Calculate the (a) mass of fluorine in the sample; (b) mass fractions of calcium and fluorine in fluorite; (c) mass percents of calcium and fluorine in fluorite.

Galena, a mineral of lead, is a compound of the metal with sulfur. Analysis shows that a 2.34-g sample of galena contains2.03 g of lead. Calculate the mass percent of lead and sulfur in galena.

Magnesium oxide (MgO) forms when the metal burns in the air. How many grams of Mg are in534 g of MgO?

Zinc sulfide (ZnS) occurs in the zinc blend crystal structure. How many kilograms of Zn are in 3.82 kg of ZnS?

A compound of copper and sulfur contains 88.39 g of metal and 44.61 g of nonmetal. How many grams of copper are in5264 kg of the compound? How many grams of sulfur?

A compound of iodine and cesium contains 63.94 g of metal and 61.06 g of nonmetal. How many grams of cesium are in38.77 g of compound? How many grams of iodine?

Show, with calculations, how the following data illustrate thelaw of multiple proportions:Compound 1: 47.5 mass % sulfur and 52.5 mass % chlorineCompound 2: 31.1 mass % sulfur and 68.9 mass % chlorine

Show, with calculations, how the following data illustrate the law of multiple proportions:Compound 1: 77.6 mass % xenon and 22.4 mass % fluorineCompound 2: 63.3 mass % xenon and 36.7 mass % fluorine

Dolomite is a carbonate of magnesium and calcium. Analysisshows that 7.81 g of dolomite contains 1.70 g of Ca. Calculate themass percent of Ca in dolomite. On the basis of the mass percentof Ca, and neglecting all other factors, which is the richer sourceof Ca, dolomite or fluorite (see Problem 2.20)?

The mass percent of sulfur in a sample of coal is a key factor in the environmental impact of the coal because the sulfur combines with oxygen when the coal is burned and the oxide can then be incorporated into acid rain. Which of the following coals would have the smallest environmental impact?

Which of Dalton’s postulates about atoms are inconsistent with later observations? Do these inconsistencies mean that Dayton was wrong? Is Dalton’s model still useful? Explain.

Use Dalton’s theory to explain why potassium nitrate from India or Italy has the same mass percents of K, N, and O.

Thomson was able to determine the mass/charge ratio of the electron but not it's mass. How did Millikan’s experiment allow the determination of the electron’s mass?

The following charges on individual oil droplets were obtained during an experiment similar to Millikan's. Determine a charge for the electron( in coulombs), and explain your answer:
$\mathbf{-}\mathbf{1}\mathbf{.}\mathbf{602}\mathbf{\times }{\mathbf{10}}^{\mathbf{19}}\mathit{C}\mathbf{;}\mathbf{-}\mathbf{4}\mathbf{.}\mathbf{806}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{C}\mathbf{;}\mathbf{-}\mathbf{8}\mathbf{.}\mathbf{010}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{A}\mathbf{;}\mathbf{-}\mathbf{14}\mathbf{.}\mathbf{42}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathit{C}$

Describe Thomson’s model of the atom. How might it account for the production of cathode rays?

When Rutherford's coworkers bombarded gold foil with particles, they obtained results that overturned the existing (Thomson) model of the atom. Explain.

Define atomic number and mass number which can vary without changing the identity of the element?

Choose the correct answer. The difference between the mass number of an isotope and its atomic number is (a)directly related to the identity of the element; (b) the number of electrons; (c) the number of neutrons; (d) the number of isotopes.

Even though several elements have only one naturally occurring isotope and atomic nuclei have whole numbers of protons and neutrons, no atomic mass is a whole number. Use the data from Table 2.2 to explain this fact.

Argon has three naturally occurring isotopes, ³⁶Ar, ³⁸Ar, and 
⁴⁰Ar. What is the mass number of each? How many protons, neutrons, and electrons are present in each?

Chlorine has two naturally occurring isotopes, ³⁵Cl and ³⁷Cl. What is the mass number of each isotope? How many protons, neutrons, and electrons are present in each?

Do both members of the following pairs have the same number of protons? Neutrons? Electrons?

Which pair(s) consist(s) of atoms with the same Z value? N value? A value?

What class of elements lies along the “staircase” line in the periodic table? How do their properties compare with those of metals and nonmetals?

Correct each of the following statements:

(a) In the modern periodic table, the elements are arranged in order of increasing atomic mass.

(b) Elements in a period have similar chemical properties.

(c) Elements can be classified as either metalloids or nonmetals.

The elements in Groups $1A\left(1\right)$ and $7A\left(17\right)$ are all quite reactive. What is the major difference between them?

Give the name, atomic symbol, and group number of the element with the following Z value, and classify it as a metal, metalloid, or nonmetal:

(a) Z = 32 (b) Z = 15 (c) Z = 2 (d) Z = 3 (e) Z = 42

Fill in the blanks:

(a) The symbol and atomic number of the heaviest alkaline earth metal are ________ and ________.

(b) The symbol and atomic number of the lightest metalloid in Group 4A(14) are ________ and ________.

(c) Group 1B(11) consists of the coinage metals. The symbol and atomic mass of the coinage metal whose atoms have the fewest electrons are________ and ________.

(d) The symbol and atomic mass of the halogen in Period 4 are ________ and ________.

What are some characteristic properties of elements to the left of the elements along the “staircase”? To the right?

Fill in the blanks:

(a) The symbol and atomic number of the heaviest nonradioactive noble gas are ________and ________.

(b) The symbol and group number of the Period 5 transition element whose atoms have the fewest protons are ________and ________.

(c) The elements in Group 6A(16) are sometimes called the chalcogens. The symbol and atomic number of the first metallic chalcogen are ________and ________.

(d) The symbol and number of protons of the Period 4 alkali metal atom are ________and ________.

Give the name, atomic symbol, and group number of the element with the following Z value, and classify it as a metal, metalloid, or nonmetal:

(a) Z = 33 (b) Z = 20 (c) Z = 35 (d) Z = 19 (e) Z = 13

How can iodine (Z = 53) have a higher atomic number yet a lower atomic mass than tellurium (Z = 52)?

Correct each of the following statements:

(a) In the modern periodic table, the elements are arranged in order of increasing atomic mass.

(b) Elements in a period have similar chemical properties.

(c) Elements can be classified as either metalloids or nonmetals.

What class of elements lies along the “staircase” line in the periodic table? How do their properties compare with those of metals and nonmetals?

What are some characteristic properties of elements to the left of the elements along the “staircase”? To the right?

The elements in Groups $\mathbf{1}\mathbf{A}\left(1\right)$ and  $\mathbf{7}\mathbf{A}\mathbf{\left(}\mathbf{17}\mathbf{\right)}$are all quite reactive. What is the major difference between them?

Give the name, atomic symbol, and group number of the element with the following Z value, and classify it as a metal, metalloid, or nonmetal:

(a) Z = 32 (b) Z = 15 (c) Z = 2 (d) Z = 3 (e) Z = 42

Give the name, atomic symbol, and group number of the element with the following Z value, and classify it as a metal, metalloid, or nonmetal:

(a) Z = 33 (b) Z = 20 (c) Z = 35 (d) Z = 19 (e) Z = 13

Fill in the blanks:

(a) The symbol and atomic number of the heaviest alkaline earth metal are ________ and ________.

(b) The symbol and atomic number of the lightest metalloid in Group 4A(14) are ________ and ________.

(c) Group 1B(11) consists of the coinage metals. The symbol and atomic mass of the coinage metal whose atoms have the fewest electrons are________ and ________.

(d) The symbol and atomic mass of the halogen in Period 4 are ________ and ________.

Fill in the blanks:

(a) The symbol and atomic number of the heaviest nonradioactive noble gas are ________and ________.

(b) The symbol and group number of the Period 5 transition element whose atoms have the fewest protons are ________and ________.

(c) The elements in Group 6A(16) are sometimes called the chalcogens. The symbol and atomic number of the first metallic chalcogen are ________and ________.

(d) The symbol and number of protons of the Period 4 alkali metal atom are ________and ________.

Describe the type and nature of the bonding that occurs between reactive metals and nonmetals.

Describe the type and nature of the bonding that often occurs between two nonmetals.

How can ionic compounds be neutral if they consist of positive and negative ions?

Given that the ions in LiF and MgO are of similar size, which compound has stronger ionic bonding? Use Coulomb’s law in your explanation.

Are molecules present in a sample of BaF₂? Explain.

Are ions present in a sample ${\mathbf{P}}_{\mathbf{4}}{\mathbf{O}}_{\mathbf{6}}$  ? Explain.

The monatomic ions of Groups 1A(1) and 7A(17) are all singly charged. In what major way do they differ? Why?

Describe the formation of solid magnesium chloride ( ${\mathbf{MgCl}}_{\mathbf{2}}$) from large numbers of magnesium and chlorine atoms.

Describe the formation of solid potassium sulfide (K₂S) from large numbers of potassium and sulfur atoms.