Chapter Questions
Which of the following of Dalton's proposals proved to be invalid?(a) Atoms are indestructible.(b) Atoms of the same element are identical.(c) Atoms can combine in more than one whole number ratio.
Which of the following of Dalton's proposals proved to be invalid?(a) Atoms of different elements combine to form compounds.(b) Atoms can combine in small whole number ratios.(c) Atoms are indivisible.
State two experimental laws Dalton used to support the atomic theory.
State three scientists whose work Dalton used to support the atomic theory.
What do the raisins represent in the plum pudding model of the atom?
What does the pudding represent in the plum pudding model of the atom?
What is the simplest negative particle in an atom?
What is the simplest positive particle in an atom?
What is the relative charge on an electron?
What is the relative charge on a proton?
Where is the location of electrons in an atom?
Where is the location of protons and neutrons in an atom?
What is the approximate size (in $\mathrm{cm}$ ) of a nucleus?
What is the approximate size (in $\mathrm{cm}$ ) of an atom?
What is the relative charge of an electron and proton?
What is the relative mass of an electron and proton?
State the number of neutrons in an atom of each of the following isotopes:(a) ${ }_{10}^{20} \mathrm{Ne}$(b) ${ }_{18}^{40} \mathrm{Ar}$(c) ${ }_{36}^{80} \mathrm{Kr}$(d) ${ }_{54}^{131} \mathrm{Xe}$
State the number of neutrons in an atom of each of the following isotopes:(a) $\quad{ }_{11}^{23} \mathrm{Na}$(b) $\quad{ }_{30}^{65} \mathrm{Zn}$(c) $\frac{27}{13} \mathrm{Al}$(d) ${ }_{47}^{107} \mathrm{Ag}$
State the number of neutrons in an atom of each of thefollowing isotopes:(a) hydrogen-1(b) carbon-13(c) cobalt-59(d) iodine-127
State the number of neutrons in an atom of each of thefollowing isotopes:(a) hydrogen-2(b) carbon-14(c) $\operatorname{cobalt}-60$(d) iodine-131
Complete the following table and provide the missing information:
Draw a diagram of the arrangement of protons, neutrons, and electrons in an atom of each of the following isotopes:(a) ${ }_{3}^{7} \mathrm{Li}$(b) ${ }_{6}^{13} \mathrm{C}$(c) ${ }_{8}^{16} \mathrm{O}$(d) ${ }_{10}^{20} \mathrm{Ne}$
Draw a diagram of the arrangement of protons, neutrons, and electrons in an atom of each of the following isotopes:(a) $^{31} \mathrm{P}$(b) $^{35} \mathrm{Cl}$(c) ${ }^{40} \mathrm{Ar}$(d) 131 I
Distinguish between atomic number and mass number.
Distinguish between atomic mass and isotopic mass.
What is the assigned mass for the current reference isotope?
What is the current atomic mass scale reference isotope?
Given that the only naturally occurring isotope of sodium is ${ }^{23} \mathrm{Na},$ determine its mass from the periodic table.
Given that the only naturally occurring isotope of aluminum is ${ }^{27} \mathrm{Al}$, determine its mass from the periodic table.
Given that the only naturally occurring isotope of fluorine is ${ }^{19} \mathrm{~F}$, determine its mass from the periodic table.
Given that the only naturally occurring isotope of phosphorus is ${ }^{31} \mathrm{P},$ determine its mass from the periodic table.
Calculate the atomic mass for lithium given the following data for its natural isotopes:$$\begin{array}{ccc}{ }^{6} \mathrm{Li} & 6.015 \mathrm{amu} & 7.42 \% \\{ }^{7} \mathrm{Li} & 7.016 \mathrm{amu} & 92.58 \%\end{array}$$
Calculate the atomic mass for magnesium given the following data for its natural isotopes:$$\begin{array}{lll}{ }^{24} \mathrm{Mg} & 23.985 \mathrm{amu} & 78.70 \% \\{ }^{25} \mathrm{Mg} & 24.986 \mathrm{amu} & 10.13 \% \\{ }^{26} \mathrm{Mg} & 25.983 \mathrm{amu} & 11.17 \%\end{array}$$
Calculate the atomic mass for iron given the following data for its natural isotopes:$$\begin{array}{llc}{ }^{54} \mathrm{Fe} & 53.940 \mathrm{amu} & 5.82 \% \\{ }^{56} \mathrm{Fe} & 55.935 \mathrm{amu} & 91.66 \% \\{ }^{57} \mathrm{Fe} & 56.935 \mathrm{amu} & 2.19 \% \\{ }^{58} \mathrm{Fe} & 57.933 \mathrm{amu} & 0.33 \%\end{array}$$
Calculate the atomic mass for zinc given the following data for its natural isotopes:$$\begin{array}{rlr}{ }^{64} \mathrm{Zn} & 63.929 \mathrm{amu} & 48.89 \% \\{ }^{66} \mathrm{Zn} & 65.926 \mathrm{amu} & 27.81 \% \\{ }^{67} \mathrm{Zn} & 66.927 \mathrm{amu} & 4.11 \% \\{ }^{68} \mathrm{Zn} & 67.925 \mathrm{amu} & 18.57 \% \\{ }^{70} \mathrm{Zn} & 69.925 \mathrm{amu} & 0.62 \%\end{array}$$
Which has the longer wavelength: red light or green light?
Which has the shorter wavelength: blue light or violet light?
Which has the lower frequency: red light or green light?
Which has the higher frequency: blue light or violet light?
Which has the lower energy: red light or green light?
Which has the higher energy: blue light or violet light?
Which wavelength has the lower frequency: $450 \mathrm{nm}$ or $550 \mathrm{nm} ?$
Which wavelength has the higher frequency: $550 \mathrm{nm}$ or $650 \mathrm{nm} ?$
What particle represents the quantum nature of light energy?
What particle represents the quantum nature of electrical energy?
State whether each of the following is continuous or quantized:(a) a rainbow(b) a line spectrum
State whether each of the following is continuous or quantized:(a) a spiral staircase(b) an elevated ramp
State whether each of the following instruments gives a continuous or a quantized measurement of length:(a) a metric ruler(b) a digital laser
State whether each of the following instruments gives a continuous or a quantized measurement of volume:(a) $10 \mathrm{~mL}$ volumetric pipet(b) $10 \mathrm{~mL}$ graduated cylinder
Draw the Bohr model of the atom.
Draw the Bohr model of the atom
What is the experimental evidence for electron energy levels in an atom?
Which of the following energy level changes for an electron is most energetic: $5 \rightarrow 2,4 \rightarrow 2,$ or $3 \rightarrow 2 ?$
Which of the following energy level changes for an electron is least energetic: $4 \rightarrow 1,3 \rightarrow 1,$ or $2 \rightarrow 1 ?$
In a hydrogen atom, what color is the emission line observed when electrons drop from the fourth to the second energy level?
In a hydrogen atom, what color is the emission line observed when electrons drop from the fifth to the second energy level?
In the emission spectrum from hydrogen gas, what type of energy is released when electrons drop from the fifth to the first energy level?
In the emission spectrum from hydrogen gas, what type of energy is released when electrons drop from the fifth to the fourth energy level?
Which of the following lines in the emission spectrum of hydrogen has the least energy: red, blue-green, or violet?
Which of the following lines in the emission spectrum of hydrogen has the shortest wavelength: red, blue-green, or violet?
How many photons of light are emitted for each of the following?(a) $1 \mathrm{e}^{-}$ drops from energy level 3 to 1(b) $1 \mathrm{e}^{-}$ drops from energy level 3 to 2
How many photons of light are emitted for each of the following?(a) $100 \mathrm{e}^{-}$ drop from energy level 3 to 2(b) $100 \mathrm{e}^{-}$ drop from energy level 4 to 2
What is the color of the spectral line emitted for each of the following electron energy changes in excited hydrogen gas?(a) Electrons drop from energy level 2 to 1(b) Electrons drop from energy level 3 to 2(c) Electrons drop from energy level 4 to 3
What is the color of the spectral line emitted for each of the following electron energy changes in excited hydrogen gas?(a) Electrons drop from energy level 5 to 1(b) Electrons drop from energy level 5 to 2(c) Electrons drop from energy level 5 to 4
What experimental evidence suggests the concept of electrons in energy levels?
What experimental evidence suggests main energy levels split into sublevels?
State the number of sublevels in each of the following main energy levels:(a) 1 st(b) 2 nd(c) $3 \mathrm{rd}$(d) 4 th
Designate all the sublevels within each of the following main energy levels:(a) 1 st(b) 2 nd(c) $3 \mathrm{rd}$(d) 4 th
What is the maximum number of electrons in each of thefollowing sublevels?(a) $2 s$(b) $4 p$(c) $3 d$(d) $5 f$
What is the maximum number of electrons in each of thefollowing?(a) an s sublevel(b) a $p$ sublevel(c) a $d$ sublevel(d) an $f$ sublevel
What is the maximum number of electrons in the second energy level?
What is the maximum number of electrons in the fourth energy level?
Draw a filling diagram and predict the sublevel that follows $4 s$.
Draw a filling diagram and predict the sublevel that follows $5 s$.
Write the predicted electron configuration for each of the following elements:(a) He(b) Be(c) Co(d) $\mathrm{Cd}$
Write the predicted electron configuration for each of the following elements:(a) boron(b) argon(c) manganese(d) nickel
Which element corresponds to each of the following electron configurations?(a) $1 s^{2} 2 s^{1}$(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}$(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{2}$(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2}$
Which element corresponds to each of the following electron configurations?(a) $1 s^{2} 2 s^{2} 2 p^{5}$(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2} 4 d^{5}$(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2} 4 d^{10} 5 p^{5}$
Sketch a three-dimensional representation for each of the following orbitals. Label the $x$ -axis, $y$ -axis, and $z$ -axis.(a) $1 s$(b) $2 p_{x}$(c) $3 P_{Y}$(d) $4 p_{z}$
Sketch a three-dimensional representation for each of the following orbital sets. Label the $x$ -axis, $y$ -axis, and $z$ -axis.(a) $1 s, 2 s, 2 p_{x}$(b) $3 p_{x}, 3 p_{Y}, 3 p_{z}$
Which orbital in each of the following pairs has the higher energy?(a) $2 s$ or $3 s$(b) $2 p_{x}$ or $3 p_{x}$(c) $2 p_{x}$ or $2 p_{y}$(d) $4 p_{\mathrm{y}}$ or $4 p_{\mathrm{z}}$
Which orbital in each of the following pairs has the larger size?(a) $2 s$ or $3 s$(b) $2 p_{x}$ or $3 p_{x}$(c) $2 p_{x}$ or $2 p_{\mathrm{y}}$(d) $4 p_{\mathrm{y}}$ or $4 p_{\mathrm{z}}$
Designate the orbital that fits each of the following descriptions:(a) a spherical orbital in the fifth energy level(b) a dumbbell-shaped orbital in the fourth energy level
Designate the orbital that fits each of the following descriptions:(a) a spherical orbital in the sixth energy level(b) a dumbbell-shaped orbital in the third energy level
State the maximum number of electrons that can occupy each of the following orbitals:(a) $1 s$(b) $2 p$(c) $3 d$(d) $4 f$
State the maximum number of electrons that can occupy each of the following sublevels:(a) $1 s$(b) $2 p$(c) $3 d$(d) $4 f$
Silver occurs naturally as ${ }^{107} \mathrm{Ag}$ and ${ }^{109} \mathrm{Ag} .$ Given the mass and abundance of silver-109 $(108.91$ amu and $48.16 \%)$, what is the isotopic mass of silver-107?
Gallium occurs naturally as ${ }^{69} \mathrm{Ga}$ and ${ }^{71} \mathrm{Ga}$. Given the mass and abundance of gallium- $69(68.92$ amu and $60.10 \%)$, what is the isotopic mass of gallium-71?
Element 43 is used in medical radiology to locate tumors. Refer to the periodic table and state whether Tc has any stable isotopes.
Element 61 was named for the mythological Greek Prometheus who stole fire from the gods. Refer to the periodic table and state whether $\mathrm{Pm}$ has any stable isotopes.
Indicate the region of the spectrum for each of the following wavelengths of light.(a) $280 \mathrm{nm}$(b) $1200 \mathrm{nm}$
Indicate the region of the spectrum for each of the following wavelengths of light.(a) $320 \mathrm{nm}$(b) $1500 \mathrm{nm}$
Bromine has only two natural isotopes, and they occur in about equal abundance. If $79 \mathrm{Br}$ is one of the isotopes, what is the other isotope given the atomic mass of bromine is approximately 80 amu?
Silver has only two natural isotopes, and they occur in about equal abundance. If $109 \mathrm{Ag}$ is one of the isotopes, what is the other isotope given the atomic mass of silver is approximately 108 amu?
Explain why the electron configuration for copper is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1} 3 d^{10}$ rather than the predicted $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{9}$.
Explain why the electron configuration for silver is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{1} 4 d^{10}$ rather than thepredicted $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2} 4 d^{9}$.
Which element is responsible for the color of rose gold?
Which element gives rise to the expression "acid test?"
Describe the glow from hydrogen in the plasma state.
Describe the color of oxygen in the liquid state.