Chemistry hw 2

Gaining electrons will fill their octet faster than losing them *Halogens form anion because they have low electron affinity.

Halogens tend to form anions because A) losing electrons will fill their octet faster than gaining them. B) gaining electrons will fill their octet faster than losing them. C) halogen element ionization energies are lower than transition metal ionization energies. D) halogen atomic radii tend to be larger than their corresponding ionic radii. E) halogen atomic radii tend to be smaller than their corresponding ionic radii.

6 *The number of atomic orbitals with a given value of n is determined by the quantum number ℓ. ℓ = 1 represents the set of p orbitals, which consists of three orbitals which can each hold two electrons, meaning that the orbitals designated by the quantum numbers n = 2, ℓ = 1 (the 2p orbitals) can contain a total of 6 electrons.

How many electrons can be assigned to orbitals designated by the quantum numbers n = 2, ℓ = 1?

10 *The number of atomic orbitals with a given value of n is determined by the quantum number ℓ. ℓ = 2 represents the set of d orbitals, which consists of five orbitals which can each hold two electrons, meaning that the orbitals designated by the quantum numbers n = 3, ℓ = 2 (the 3d orbitals) can contain a total of 10 electrons.

How many electrons can be assigned to orbitals designated by the quantum numbers n = 3, ℓ = 2?

n = 3, ℓ = 2, mℓ = -2 *A d orbital is represented by the quantum number ℓ = 2 ( s = 0, p = 1, d = 2, f = 3). The only option that meets this criterion is the set n = 3, ℓ = 2, mℓ = -2.

An electron is shown to occupy a d orbital. Which of the following sets of quantum numbers can describe this electron?

The true nuclear charge minus the charge that is shielded by the electrons

Effective nuclear charge, Zeff, is defined as A) the number of protons minus the number of valence electrons. B) the difference in electronegativities of two bonded atoms or ions. C) the number of protons minus the number of electrons. D) the true nuclear charge minus the charge that is shielded by electrons. E) the number of protons in the nucleus.

3p *Atomic orbitals are described by their principal quantum number (n) followed by a letter that corresponds to the value for the angular momentum quantum number (ℓ). Here, n = 3, so the atomic orbital symbol will begin with 3. The quantum number ℓ = 1 (s = 0, p = 1, d = 2, f = 3), which corresponds to p. Therefore, this is a 3p atomic orbital.

For which atomic orbital does n = 3 and ℓ = 1?

small wavelength *The relationship between energy and wavelength is shown. E = hc/λ If the energy is high that means the wavelength will be small/short.

If light has a lot of energy, it will have:

1 *The following solution may contain one or more values that are different from the problem provided to you, however, the steps to solve the problem are the same. .According to the rules governing acceptable quantum numbers, the value for ℓ can only be as high as n-1. If n = 2, the maximum value for ℓ is 1.

If n = 2, what is the maximum allowed value for ℓ?

n = 6 *The value for mℓ must be between -ℓ and ℓ, so if ℓ = 0, mℓ must 0 as well. The value for ms must be either +1/2 or -1/2, so it cannot be 1 or 0. The value of ℓ must be less than the value of n, so ℓ = 0 and n = 6 is acceptable.

If ℓ = 0, which of the following may be true?

4f *The energy of an electron is primarily dictated by its principal quantum number, n. For atoms with multiple electrons, electrons that have the same value of n (as is the case here, with n = 4) will have higher energies with higher values of ℓ. Of these options, the 4f orbital has the highest value of ℓ (ℓ = 3), so it will have the highest energy.

In a multi-electron atom, which orbital will have the highest energy?

Down and to the left

In which direction on the periodic table does metallic character increase? A) Down and to the right. B) Down and to the left. C) As you move toward the middle of the table. D) Up and to the right. E) Up and to the left.

wave B *All light travels at the same speed (c), and since speed is equal to the product of wavelength and frequency, a higher frequency results in a shorter wavelength. Because wave A has a greater frequency than wave B, wave B must have the longer wavelength.

Light wave A has a greater frequency than light wave B. Which has a greater wavelength?

F > Be > Li > Ba *In general, first ionization energy decreases down a group and increases across a period.

Rank the following atoms in order of decreasing first ionization energies (i.e., highest to lowest): Li, Be, Ba, F. A) Ba > Li > Be > F B) F > Be > Li > Ba C) Li > Be > F > Ba D) F > Be > Ba > Li E) Ba > F > Be > Li

O < Be < Li < Al < Ba *In general, atomic radius decreases across a period and increases down a group.

Rank the following atoms in order of increasing size (i.e., smallest to largest): Li, Al, Be, Ba, O. A) Li < Al < Be < Ba < O B) Ba < Al < Li < Be < O C) Li < Be < O < Al < Ba D) O < Be < Li < Al < Ba E) O < Li < Be < Ba < Al

lower, longer *The electromagnetic spectrum shows that red light has a longer wavelength than ultraviolet rays. The relationship between wavelength and frequency is shown. c=λν Wavelength and frequency are inversely related, so if it has a longer wavelength than ultraviolet rays, it also has a shorter frequency than ultraviolet rays.

Red light has a _____ frequency and a _____ wavelength than ultraviolet rays.

electron affinity *The electron affinity is the change in energy when an electron is added to a neutral gaseous atom to form an ion.

The energy released in the reaction F(g) + e⁻ → F⁻(g) is known as the

True *The Pauli exclusion principle states that no two electrons in a given atom can share the same set of four quantum numbers (n, ℓ, mℓ, ms). Two electrons may share the first three quantum numbers (n, ℓ, mℓ) as long as their ms (spin) quantum numbers are not the same, so this statement is true.

True or false: two electrons can simultaneously occupy the same (n,ℓ,mℓ) orbital.

Francium (Fr) *Atomic radius increases as you move down the periodic table and to the left. Francium is the furthest down and to the left of this group and would be predicted to to be the largest element of the whole periodic table.

What element is theoretically the largest of all on the periodic table? A) Francium (Fr) B) Helium (He) C) Hydrogen (H) D) Lead (Pb) E) Radon (Ra)

1s²2s²2p⁶3s²3p⁶ *The element K is in the first column of the periodic table (meaning it is in the s block) and the fourth row, so its electron configuration will end with 4s¹. The electron configuration of K is 1s²2s²2p⁶3s²3p⁶4s¹. However, the K⁺ ion has one fewer electron (due to its positive charge), so the highest-energy electron must be removed from K to create K⁺, meaning its electron configuration will be 1s²2s²2p⁶3s²3p⁶.

What is the electron configuration of K⁺? A) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶ B) 1s²2s²2p⁶3s²3p⁶ C) 1s²2s²2p⁶3s²3p⁶4s² D) 1s²2s²2p⁶ E) 1s²2s²2p⁶3s²3p⁵

Kr *The noble gas core for a given element is the last noble gas filled in the periodic table prior to the given element. Here, the last noble gas prior to Ru is Kr, so that is its noble gas core.

What is the noble gas core in the electron configuration for Ru?

Rn *The noble gas core for a given element is the last noble gas filled in the periodic table prior to the given element. Here, the last noble gas prior to U is Rn, so that is its noble gas core.

What is the noble gas core in the electron configuration for U?

Hund's Rule

What quantum mechanics principle states that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having the same spin? A) Schrödinger's equation B) Heisenberg uncertainty principle C) Pauli exclusion principle D) Aufbau principle E) Hund's rule

Mn *This electron configuration ends with 3d, meaning it is an element in the d block. Because elements in the d block have the quantum number n one less than their row in the periodic table, this element will be in the fourth row. Because it ends in 3d⁵, it will be the fifth element in the fourth row d block, meaning it must be Mn.

Which element has the electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d⁵?

Cr *This electron configuration ends with 3d, meaning it is an element in the d block. Because elements in the d block have the quantum number n one less than their row in the periodic table, this element will be in the fourth row. While the 5 in 3d⁵ normally indicates that this electron configuration corresponds to the fifth entry in that row, the 4s orbital is only half-filled (with 1 electron instead of 2); if the 4s orbital were filled, it would take an electron from the 3d orbital, so 4s¹3d⁵ would change to 4s²3d⁴. This would correspond to the fourth element in that row, which is Cr. The reason the electron configuration of Cr ends in 4s¹3d⁵ instead of 4s²3d⁴ is that having two half-filled orbitals is more stable than having one partially filled (but not exactly half-filled) and one completely filled.

Which element has the electron configuration 1s²2s²2p⁶3s²3p⁶4s¹3d⁵?

Sb (Antimony) *This electron configuration ends with 5p, meaning it is an element in the p block (a main group element on the right-hand side of the periodic table) in the fifth row. The 3 in 5p³ indicates that it is the third element in this row, so the element must be Sb.

Which element has the ground state electron configuration [Kr]5s²4d¹⁰5p³?

W (Tungsten) *This electron configuration ends with 5d, meaning it is an element in the d block. Because elements in the d block have the quantum number n one less than their row in the periodic table, this element will be in the sixth row. The 4 in 5d⁴ indicates that it is the fourth element in this row, so the element must be W.

Which element has the ground state electron configuration [Xe]6s²4f¹⁴5d⁴?

gamma rays *The relationship between wavelength and frequency is shown. c=λν Wavelength and frequency are inversely related, so the shortest wavelength would have the highest frequency. The electromagnetic spectrum shows that gamma rays have the smallest wavelength, and therefore the highest frequency.

Which of the following forms of radiation has the highest frequency?

Metals *cation = a positively charged ion, i.e. one that would be attracted to the cathode in electrolysis.

Which of the following groups of elements tend to form cations? A) Metals B) Metalloids C) Nonmetals D) Noble gases E) Radioactive elements

Each successive ionization requires increasing amounts of energy *Each successive ionization of an atom and its ions requires increasing amounts of energy to remove the electrons.

Which of the following is true concerning successive ionizations of an atom and its ions? A) Each successive ionization requires less energy to achieve. B) All ionizations require the same amount of energy. C) The amount of energy required to achieve a successive ionization doubles with each electron removed. D) Each successive ionization requires increasing amounts of energy. E) The first two ionizations are endothermic but each ionization afterwards is exothermic.

Tantalum (Ta) *The atomic radius increases as you move down the periodic table and to the left. Tantalum is the furthest to the right of this list and nearer the top and it would be expected to have the smallest atomic radius.

Which of the following metals would be expected to have the smallest atomic radius? A) Cesium (Cs) B) Barium (Ba) C) Lanthanum (La) D) Europium (Eu) E) Tantalum (Ta)

Mg²⁺ and O²⁻ *Isoelectronic species are elements/ions with the same electron configuration (and therefore the same number of electrons). Of the options given, the species Mg²⁺ and O²⁻ both have the electron configuration of Ne (1s²2s²2p⁶), meaning they are isoelectronic.

Which of the following pairs of ions represent isoelectronic species? A) Mg²⁺ and O²⁻ B) K+ and Li+ C) Ca²⁺ and F- D) Fe²⁺ and S²⁻ E) Al³⁺ and Cl⁻

1s²2s²2p⁶3s²3p⁶ *The element P is a main-group element on the right-hand side of the periodic table (meaning it is in the p block) and the third row, so its electron configuration will end with 3p. The electron configuration of P is 1s²2s²2p⁶3s²3p³. However, the P³⁻ ion has three additional electrons (due to its charge of 3-), so three electrons must be added to the atom, resulting in the electron configuration 1s²2s²2p⁶3s²3p⁶.

Which of the following represents the electron configuration of P³⁻? A) 1s²2s²2p⁶3s²3p⁶ B) 1s²2s²2p⁶3s²3p³ C) 1s²2s²2p⁶3s² D) 1s²2s²2p⁶3s²3p⁶4s¹ E) 1s²2s²2p⁶3s²3p¹

n = 3, ℓ = 1, mℓ = 1 *Atomic orbitals are described by their principal quantum number (n) followed by a letter that corresponds to the value for the angular momentum quantum number (ℓ). For a 3p electron, the number 3 represents n, whereas s represents ℓ. ℓ corresponds to the following values: s = 0, p = 1, d = 2, f = 3; this means that in this orbital, ℓ = 1. The value for mℓ must be between -ℓ and ℓ, so if ℓ = 1, mℓ must be -1, 0, or 1.

Which of the following sets of quantum numbers can describe a 3p electron?

n = 4, ℓ = 0, mℓ = 0 *Atomic orbitals are described by their principal quantum number (n) followed by a letter that corresponds to the value for the angular momentum quantum number (ℓ). For a 4s electron, the number 4 represents n, whereas s represents ℓ. ℓ corresponds to the following values: s = 0, p = 1, d = 2, f = 3; this means that in this orbital, ℓ = 0. The value for mℓ must be between -ℓ and ℓ, so if ℓ = 0, mℓ must be 0 as well.

Which of the following sets of quantum numbers can describe a 4s electron?

n = 3, ℓ = 0, mℓ = 0 *The orbital shown in this figure is spherical, meaning it has no angular nodes. Because the number of angular nodes is equal to the quantum number ℓ, this implies that ℓ = 0, meaning this is an s-orbital. The only option that meets this criterion is the set n = 3, ℓ = 0, mℓ = 0.

Which of the following sets of quantum numbers could describe an electron in the orbital shown below?

n = 2, ℓ = 2, mℓ = 2 *According to the rules governing acceptable quantum numbers, the value for ℓ can only be as high as n-1, so the value of ℓ cannot equal the value of n. Therefore, the set {n = 2, ℓ = 2, mℓ = 2} is not allowed.

Which of the following sets of quantum numbers is not allowed?

Pauli Exclusion Principle

Which of the following states that no two electrons can have the same set of four quantum numbers? A) Hund's rule B) de Broglie wave equation C) Pauli exclusion principle D) Bohr equation E) Schrödinger equation

(3,0,1) *The value for mℓ must be between -ℓ and ℓ, so if ℓ = 0, mℓ must 0 as well. As such, the quantum state (n = 3, ℓ = 0, mℓ = 1) is not possible.

Which quantum state (n,ℓ,mℓ) is NOT possible?

Radio waves *The electromagnetic spectrum shows that radio waves have the longest/largest wavelength.

Which type of electromagnetic radiation has the largest wavelength?