Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

An unknown particle is caused to move between two electrically charged plates, as illustrated in Figure 2.8. Its path is deflected by a smaller magnitude in the opposite direction from that of a beta particle. What can you conclude about the charge and mass of this unknown particle?Figure 2.8
How did Rutherford interpret the following observations made during his α-particle scattering experiments? (a) Most α particles were not appreciably deflected as they passed through the gold foil. (b) A few α particles were deflected at very large angles. (c) What differences would you expect if
Millikan determined the charge on the electron by studying the static charges on oil drops falling in an electric field (Figure 2.5). A student carried out this experiment using several oil drops for her measurements and calculated the charges on the drops. She obtained the following data:Droplet
The radius of an atom of gold (Au) is about Å. (a) Express this distance in nanometers (nm) and in picometers (pm). (b) How many gold atoms would have to be lined up to span 1.0 mm? (c) If the atom is assumed to be a sphere, what is the volume in cm3 of a single Au atom?
An atom of rhodium (Rh) has a diameter of about 2.7 × 10-8. (a) What is the radius of a rhodium atom in angstroms (Å) and in meters (m)? (b) How many Rh atoms would have to be placed side by side to span a distance of 6.0 μm? (c) If you assume that the Rh atom is a sphere, what is the volume in
Answer the following questions without referring to Table 2.1:(a) What are the main subatomic particles that make up the atom?(b) What is the relative charge (in multiples of the electronic charge) of each of the particles?(c) Which of the particles is the most massive?(d) Which is the least
The following diagram is a representation of 20 atoms of a fictitious element, which we will call nevadium (Nv). The red spheres are 293Nv, and the blue spheres are 295Nv.(a) Assuming that this sample is a statistically representative sample of the element, calculate the percent abundance of each
Determine whether each of the following statements is true or false. If false, correct the statement to make it true: (a) The nucleus has most of the mass and comprises most of the volume of an atom. (b) Every atom of a given element has the same number of protons. (c) The number of electrons in an
(a) Define atomic number and mass number. (b) Which of these can vary without changing the identity of the element?
(a) Which two of the following are isotopes of the same element: ? (b) What is the identity of the element whose isotopes you have selected?
How many protons, neutrons, and electrons are in the following atoms: (a) 40Ar (b) 65Zn (c) 70Ga (d) 80Br (e) 184W (f) 243Am?
Each of the following isotopes is used in medicine. Indicate the number of protons and neutrons in each isotope: (a) Phosphorus- 32 (b) Chromium-51 (c) Cobalt-60 (d) Technetium- 99 (e) Iodine-131 (f) Thallium-201.
Fill in the gaps in the following table, assuming each column represents a neutral atom.
Fill in the gaps in the following table, assuming each column represents a neutral atom.
One way in which Earth's evolution as a planet can be understood is by measuring the amounts of certain isotopes in rocks. One quantity recently measured is the ratio of 129Xe to 130Xe in some minerals. In what way do these two isotopes differ from one another? In what respects are they the same?
(a) What isotope is used as the standard in establishing the atomic mass scale? (b) The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of 10.81 amu. Explain.
(a) What is the mass in amu of a carbon-12 atom? (b) Why is the atomic weight of carbon reported as 12.011 in the table of elements and the periodic table in the front inside cover of this text?
Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass = 84.9118 amu; abundance = 72.15% and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85%. Calculate the atomic weight of rubidium.
(a) In what fundamental way is mass spectrometry related to Thomson's cathode-ray experiments (Figure 2.4)?(b) What are the labels on the axes of a mass spectrum?(c) To measure the mass spectrum of an atom, the atom must first lose one or more electrons. Why is this so?Figure 2.4
(a) The mass spectrometer in Figure 2.12 has a magnet as one of its components.What is the purpose of the magnet?(b) The atomic weight of Cl is 35.5 amu. However, the mass spectrum of Cl (Figure 2.13) does not show a peak at this mass. Explain.(c) A mass spectrum of phosphorus (P) atoms shows only
Naturally occurring magnesium has the following isotopic abundances:(a) What is the average atomic mass of Mg? (b) Sketch the mass spectrum of Mg.
Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of H2 is taken under conditions that prevent decomposition into H atoms. The two
For each of the following elements, write its chemical symbol, locate it in the periodic table, give its atomic number, and indicate whether it is a metal, metalloid, or nonmetal: (a) Chromium (b) Helium (c) Phosphorus (d) Zinc (e) Magnesium (f) Bromine (g) Arsenic.
Locate each of the following elements in the periodic table; give its name and atomic number, and indicate whether it is a metal, metalloid, or nonmetal: (a) Li (b) Sc (c) Ge (d) Yb (e) Mn (f) Sb (g) Xe.
For each of the following elements, write its chemical symbol, determine the name of the group to which it belongs (Table 2.3), and indicate whether it is a metal, metalloid, or nonmetal:(a) Potassium(b) Iodine(c) Magnesium(d) Argon(e) Sulfur.Table 2.3
Does the following drawing represent a neutral atom or an ion? Write its complete chemical symbol including mass number, atomic number, and net charge (if any).
What can we tell about a compound when we know the empirical formula? What additional information is conveyed by the molecular formula? By the structural formula? Explain in each case.
Two compounds have the same empirical formula. One substance is a gas, whereas the other is a viscous liquid. How is it possible for two substances with the same empirical formula to have markedly different properties?
Write the empirical formula corresponding to each of the following molecular formulas: (a) Al2Br6 (b) C8H10 (c) C4H8O2 (d) P4O10 (e) C6H4C12 (f) B3N3H6.
Determine the molecular and empirical formulas of the following: (a) The organic solvent benzene, which has six carbon atoms and six hydrogen atoms; (b) The compound silicon tetrachloride, which has a silicon atom and four chlorine atoms and is used in the manufacture of computer chips; (c) The
Write the molecular and structural formulas for the compounds represented by the following molecular models:(a)(b) (c) (d)
Write the molecular and structural formulas for the compounds represented by the following models:(a)(b) (c) (d)
Fill in the gaps in the following table:
Which of the following diagrams most likely represents an ionic compound, and which represents a molecular one? Explain your choice.
Fill in the gaps in the following table:
Predict the chemical formula for the ionic compound formed by (a) Ca2+ and Br ¯ (b) K+ and CO3 2- (c) Al3+ and CH3COO¯ (d) NH4+ and SO42- (e) Mg2+ and PO43-.
Predict the chemical formulas of the compounds formed by the following pairs of ions: (a) Cr3+ and Br- (b) Fe3+ and O2- (c) Hg2 2+ and CO32- (d) Ca2+ and CIO3 (e) NH4 + and PO43-.
Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair.
Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair.
Predict whether each of the following compounds is molecular or ionic: (a) B2H6 (b) CH3OH (c) LiNO3 (d) Sc2O3 (e) CsBr (f) NOCl (g) NF3 (h) Ag2SO4.
Which of the following are ionic, and which are molecular? (a) PF5 (b) NaI (c) SCl2 (d) Ca(NO3)2 (e) FeCl3 (f) LaP (g) CoCO3 (h) N2O4.
Give the names and charges of the cation and anion in each of the following compounds: (a) CaO (b) Na2SO4 (c) KClO4 (d) Fe(NO3)2 (e) Cr(OH)3.

Showing 400 - 500 of 442

1
2
3
4
5

Step by Step Answers