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introductory chemistry atoms first
Introductory Chemistry Atoms First 5th Edition Steve Russo And Michael Silver - Solutions
What is wrong with this Bohr model of the beryllium (Be) atom (atomic number 4)? n = 3 n = 2 n = 1 4 p
The hydrogen atom has three other visible lines in its line spectrum: green, blue, and indigo/violet. Use the energy-level diagram for hydrogen and Table 4.1 to determine the electron jumps responsible for these lines. Indigo/ Blue violet Green Red n = 3n = 2
Using dots to represent potassium’s 19 electrons, fill the subshells in the diagram below to arrive at the ground-state energy- level diagram for the potassium atom. Select the diagram that gives an answer consistent with the periodic table. Shells n = 4 n = 3 n = 2 n = 1 Increasing
Why did Bohr split shells into subshells called s, p, d, and f?(a) To make chemistry complicated and harder for students to master.(b) To abide by the Uncertainty Principle.(c) To explain that “single” lines in a line spectrum were actually often made up of very closely spaced lines.(d) To
Draw a Bohr model for an atom of sulfur (S). How many additional electrons can fit into the n = 3 shell?
The following statement(s) is true about the periodic table:(a) Elements in the same group have similar valence-shell electron configurations.(b) Elements in the same period have the same value of n for their valence electrons.(c) When traversing an nth period in the d block, it is the (n – 1)d
Redraw the shells of Li, Be, B, and C shown in the above drawing to make the overall size of each atom fit the size trend. In each nucleus, write the total number of protons present. Which atom would be most difficult to ionize? n = 2 n=1 Lithium (Li) n=2 n=1 n =
Why is an electron in a shell that has a low value of n in a more stable arrangement than one in a shell that has a higher value of n?
When you move from left to right across a period, atoms (a) Shrink because the quantum number n increases.(b) Grow because the number of protons in the nucleus increases.(c) Shrink because the number of protons in the nucleus increases.(d) Shrink because quantization becomes smaller.
How many electrons can the n = 5 shell in an atom hold?
Locate the elements in group VIIA in the ionization energy plot. Do any of these elements violate the expected trend in ionization energies?
The ground state for the lithium (Li) atom and the scaled energies of its shells are shown below. Draw a Bohr diagram for the lowest-energy excited state of lithium. n = 3 9.00 eV. n = 2 7.75 eV. n = 1 1.00 eV- n = 3 n = 2 n = 1 Energy-level diagram 3P Bohr diagram
Ionization energy increases left to right across a period because (a) It does not. Ionization energy decreases left to right across a period.(b) As you go down a group, atoms increase in size due to increasing values of n.(c) Atoms shrink in size, resulting in a more positive nucleus and a tighter
The octet rule says which of the following?(a) Main group metals will typically lose all their valence electrons in a chemical reaction.(b) Main group nonmetals will typically gain a negative charge equal to 8 – (group number).(c) Atoms will react to achieve eight electrons in their valence
Draw a Bohr diagram for the highest-energy excited state you can make using the three shells shown in Practice Problem 4.9 and exciting only a single electron.Data from Problem 4.9The ground state for the lithium (Li) atom and the scaled energies of its shells are shown below. Draw a Bohr diagram
Draw a Bohr diagram for a Li+ cation in its ground state.
An atom has atomic number 6 and has eight electrons.(a) Which element is this?(b) Is this a neutral atom, a cation, or an anion? If it is an ion, what is its charge?(c) Draw a Bohr diagram for this atom in its ground state.
An F– anion has ten electrons. A student draws the following ground-state Bohr diagram for this anion. There are two things wrong with the diagram. What are they? n = 3 n = 2 n = 1 9P
Use electron-configuration notation to show how electrons are distributed in a ground-state silicon (Si) atom. How many valence electrons does this atom have?
Without looking at a periodic table, use electron-configuration notation to show how electrons are distributed in a ground-state atom with 33 electrons. How many valence electrons does this atom have? What periodic table group would you expect to find it in? Now look at a periodic table and
Use electron-configuration notation to show how electrons are distributed in a ground-state scandium (Sc) atom.
Using a four-block periodic table as a guide, determine the ground-state electron configuration of copper (Cu).
Using a four-block periodic table as a guide, determine the ground-state electron configuration of krypton (Kr). Explain why it is proper for this element to be in group VIIIA.
Using a four-block periodic table as a guide, determine the ground-state electron configuration of palladium (Pd).
Write the ground-state electron configuration of chlorine (Cl) and lutetium (Lu), using both the full notation and the noble gas abbreviated notation.
Write the ground-state electron configuration of radium (Ra), using both the full notation and the noble gas abbreviated notation.
What was the experimental evidence that supported the existence of subshells? Explain how this evidence suggested subshells.
(a) What is the numbering system used to label shells?(b) What is the lettering system used to label subshells?(c) How many subshells are there in a given shell?
How many electrons can each subshell hold before it is considered full?
You have seen that the 4s subshell fills before the 3d subshell. This being true, what would be wrong with drawing the Bohr diagram as follows? NO 1s
Bohr solved the potassium problem by putting its last electron where? How did he justify this?
Write the electron configuration for the following elements without using the noble gas abbreviated form (use the periodic table to assist you).(a) B (b) Sc (c) Co (d) Se (e) Ru
Repeat Problem 4.84, but use the noble gas abbreviated form this time.Data from Problem 4-84Write the electron configuration for the following elements without using the noble gas abbreviated form (use the periodic table to assist you).(a) B (b) Sc (c) Co (d) Se (e) Ru
Write the electron configuration for the following elements without using the noble gas abbreviated form.(a) Ba (b) W (c) Pb (d) Pr (e) Pa
In which period and group in the periodic table are these atoms found? (a) 1s²2s²2p³ (b) 1s²2s²2p63s¹ (c) 1s²2s²2p 3s²3p64s²3d¹04p5
Repeat Problem 4.86, but use the noble gas abbreviated form this time.Data from Problem 4-86Write the electron configuration for the following elements without using the noble gas abbreviated form.(a) Ba (b) W (c) Pb (d) Pr (e) Pa
A student has written what he thinks are some ground-state electron configurations. Which ones have something wrong with them? What is wrong?(a) 1s22p63s1 (b) 1s22s63s23p64s24p6(c) 2s22p63s23p64s23d7 (d) 1s22s22p73s33p6(e) 1s22s22p53s1(f) 1s22s22p63s23p64s23d104p65s14d4 [This is the transition
How many valence electrons does each of these atoms have?(a) 1s22s22p3 (b) 1s22s1 (c) 1s22s22p63s23p64s23d7(d) 1s22s22p63s23p6 (e) 1s2
Regarding primary quantum number n, which representative elements have valence electrons with an n value that is three times the n value of lithium’s valence electrons? What period are they in?
Write electron configurations for O, O2+ , and O2–. Which form would you expect to find in most compounds of oxygen? Why?
When using the periodic table to assign electron configurations, what is the rule for the n quantum number when you are in the d block? When you are in the f block?
Why are the s, p, d, and f blocks in the periodic table 2, 6, 10, and 14 blocks wide, respectively?
(a) According to the Bohr model, why might someone expect that atoms would not change in size as you go from left to right across a period?(b) In fact, atoms do change in size across a period. What is the trend and what is the explanation for it?
According to the Bohr model, why do atoms get larger as you proceed down a group in the periodic table?
Which atom has a smaller 1s subshell, lithium (Li) or beryllium (Be)? Justify your answer.
Which atom has a smaller valence shell, lithium (Li) or sodium (Na)? Explain your answer.
Which atom is larger, lithium (Li) or beryllium (Be)? Explain your answer.
Which atom is larger, lithium (Li) or sodium (Na)? Explain your answer.
Rank the following atoms from smallest to largest: Si, Mg, Rb, Na.
As you move from left to right across a period you add more subatomic particles to the atoms, and yet the atoms become smaller.(a) What subatomic particles are you adding?(b) If you are adding particles, why don’t the atoms become larger?
Order the following atoms from smallest to largest, judging from their relative positions in the periodic table: Cs, Fe, Ti, Hf.
Order the following atoms from smallest to largest, judging from their relative positions in the periodic table: Ca, Se, F, S.
Explain the trends in ionization energy in terms of the trends in atomic aize.
What is the octet rule, and what is the justification behind it?
How do metal atoms usually attain an octet in chemical reactions?
How do nonmetal atoms usually attain an octet in chemical reactions?
Draw the Bohr model for a Cl atom and for a Cl– ion. How many electrons are there in the valence shell in each drawing?
Draw a Bohr model for an Al atom and for an Al3+ ion. How many electrons are there in the valence shell in each drawing?
Predict the formula of the compound that forms when sodium atoms react with sulfur atoms. Completely explain your reasoning.
Predict the formula of the compound that forms when lithium atoms react with nitrogen atoms. Completely explain your reasoning.
Why are roman-numeral group numbers for the representative elements useful in predicting how many electrons an atom will gain or lose in a chemical reaction?
Consider the following Bohr diagrams for two reactants:(a) What are the identities of the two elements reacting with each other? Give full atomic symbols.(b) Which is the metal, and which is the nonmetal?(c) What is the formula of the resulting compound?(d) Draw Bohr diagrams for the ions formed. n
When a group IIA element X reacts with a group VIIA element Y, what will be the formula? Why?
Explain what is meant by this statement: The element hydrogen is an exception to the octet rule and yet it obeys it in principle.
Aluminum forms compounds with both sulfur and oxygen. Why are the formulas of the resulting compounds Al2S3 and Al2O3, respectively? Why are the formulas similar?
True or false? The O2– and F– anions have identical electron configurations. Justify your answer with Bohr diagrams and electron configuration notation.
Which part of the following statement is true and which part is false? Mg2+ and Na+ have identical electron configurations, and they also have similar properties. Explain your answer fully.
How can you tell how many electrons a representative metal is likely to lose? What, in general, will be the charge of the cation it forms?
How can you tell how many electrons a representative nonmetal is likely to gain? What, in general, will be the charge of the anion it forms?
Consider an anion and a cation joining to form a compound.(a) How does knowing the charge of the ions help to determine the formula?(b) What would be the formula of the compound formed from Ca2+ cations and N3– anions?
What is wrong with Bohr’s planetary model of atomic electrons according to modern quantum mechanical theory?
Quantum mechanical tunneling is one consequence of quantum theory. What is quantum mechanical tunneling?
Draw an s orbital, a p orbital, and a d orbital.
Suppose you could see orbitals (electron clouds) inside an atom. According to Schrödinger, describe what you would see as a 1s electron was excited to become a 2p electron.
What gave Schrödinger justification to think of an electron in an atom as a nebulous cloud?
How many seconds does it take light to travel 3.00 × 103 miles from New York to California? [1 mile = 1.61 km]
A laser emits a beam of green light that has a wavelength of 5.00 × 10–5 cm. What is the wavelength of this light in nanometers?
What is the wavelength in nanometers of infrared light for which l = 2.50 × 10–5 m? How many times longer is this wavelength than red light that has a wavelength of 750 nm?
Fill in the table: Wavelength (m) 7.85 x 10-12 m Wavelength (nm) 2602.0 nm Energy (J) 5.65 × 10-18 J
Electromagnetic radiation emitted by magnesium has a wavelength of 285.2 nm. (a) Is this radiation visible to the eye?(b) What is the energy of this radiation?
Would moving an electron farther from an atom’s nucleus give off light energy or require the absorption of light energy? Explain your answer.
Convert this excited boron, B, atom to (a) An excited state of lower energy (b) The ground state: 33 СС i сл р n = 3 n=2 n = 1
According to Bohr’s model, is energy absorbed or released when an electron moves to a shell of lower n?
According to Bohr’s model, energy must be put into an atom to move an electron from a low-energy shell to a higher-energy shell. How do you calculate the amount of energy needed for the move?
According to Bohr, what is so special about the valence shell of an atom?
What are the wavelength in nanometers and energy in joules of the light emitted when a hydrogen electron originally in the n = 6 shell relaxes to the ground state? [1 eV = 1.602 × 10–19 J]
These energy-level diagrams are for iron, Fe. Indicate whether each represents the ground state, an excited state, or is incorrect. Explain your answers. Increasing energy 1s (a) 4s 1s (b) 2s 1s (c)
Use electron configuration notation to explain why aluminum, Al, and gallium, Ga, have similar chemical properties even though gallium has d electrons but aluminum does not.
Name each element and tell how many valence electrons it has:(a) 1s22s22p63s23p2(b) [Ne]3s1(c) [Ar]4s23d104p3
Which subshell is filled in transition metals? What is unique about its order of filling?
Consider the anion whose charge is 2– and whose electron configuration is identical to that of argon, Ar. What is the symbol for this anion?
What do F–, O2– , Na+, and Mg2+ all have in common?
Why is the formula for calcium sulfide CaS and not Ca2S?
Select the element from each pair expected to have the lower first ionization energy. Explain.(a) N and F (b) Mg and Ba (c) N and Ca
How does the first ionization energy of the alkali metal in a given period compare with the first ionization energy of the halogen in the same period? What is the result in terms of how these elements tend to react with each other?
Arrange calcium, strontium, arsenic, bromine, and chlorine in order of(a) Increasing atomic size (b) Increasing first ionization energy.
Of the atoms Na, Cl, K, Br, which has the largest atomic radius? Which has the largest first ionization energy?
Arrange Ca, Se, F, S, and Rb in order of increasing ionization energy.
Predict the formula for lithium nitride, made from lithium, Li, and nitrogen, N. Explain your reasoning.
Suppose the 3s valence electron in a ground-state sodium atom is excited to the 4s orbital. Why does the electron now have higher energy?
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