Chapter 3 Homework SPC

Which will have the shortest wavelength for a given energy?

1. electron 2. hydrogen atom 3. bacterium 4. baseball answer: baseball - The greater the mass of an object, the shorter its wavelength, as they are inversely proportional. So macroscopic objects have incredibly tiny wavelengths that are negligible, unlike subatomic particles.

The 5p orbitals fill immediately after the 4d orbitals and immediately before the 6s based on: (select all that apply)

1. obsrved experimental results 2. theortical caulculations - The 5p orbitals fill immediately after the 4d orbitals and immediately before the 6s based on observed experimental results, and has been supported by theoretical calculations.

The wavelength of a particle depends on:

1. particle mass 2. particles velocity 3. plancks constant

Calculate the wavelength of an electron traveling at 6.75×106 ms if its mass is 9.11×10−31 kg. Use 6.626×10−34kg m2s for Planck's constant.

1.08×10^-10 m

What is the wavelength of an electron (9.11×10−31 kg) traveling at 5.00×106ms? Use 6.626×10−34kg m2s for Planck's constant.

1.45×10−10 m

The water in a garden hose flows at a rate of 10.0 liters per minute. What is the flow rate in gallons per hour? (1gal=3.79L)

158

What is the electron configuration for O2−?

1s2, 2s2, 2p6 - The O anion gains 2 electrons so 1s22s22p6 from 1s22s22p4.

What is the electron configuration for K+?

1s2, 2s2, 2p6, 3s2, 3p6 - k loses an electron so it. moves from 4s to 3p

What is the wavelength of a baseball with a mass of 150. g and a velocity of 22.0 ms? Use 6.626×10−34kg m2s for Planck's constant.

2.00 x 10^-34

Tyson Gay's best time to run 100.0 meters (m) was 9.69 seconds (s). What was his average speed during this run, in miles per hour (mph)? (3.281feet=1 meter)(1 mile=5280 feet)

23.1

Which would be an invalid listing within an electron configuration?

2d5

How many electrons can the n=4 energy level hold?

32 s hold 2 p hold 6 d hold 10 f hold 14

In polyelectronic atoms, the orbitals that are next highest in energy after the 4s orbital are the:

3d

What is the frequency, in Hertz, of an electromagnetic wave with a wavelength of 625 nm?

4.80×1014 Hz

The orbitals that are usually the next highest in energy after the 6s orbitals are the:

4f - The f orbitals are two behind the period number in terms of principal quantum number.

What is the wavelength of radiation with a frequency of 6.0×1015 Hz?

5.0×10−8 m

A certain kind of light has a wavelength of 4.6 μm (micrometers). What is the frequency of this light in GHz?

6.5 x 10^4

What is the wavelength of a wave with a frequency of 4.3 Hz?

6.97 x 10^7

Which subshell holds the valence electrons of barium?

6s

Which of the following may contribute to the increased radius of an anion compared to parent atom?

Additional electrons lead to more electron-electron repulsion, which will increase the average distances of all the outer orbitals from the nucleus. - Anions are larger than their parent atoms due to the additional electrons. Since electrons are all negatively charged, they all repel each other and spread further apart, increasing the radius of the ion. The charge of the nucleus does not change because anions are not formed by changing the number of protons in the nucleus - only by changing the number of electrons. The *effective* nuclear charge may decrease, but this is a form of electron-electron repulsion.

Which of the following is the correct sequence for increasing order (i.e., smallest to largest) of first ionization energy (IE)?

B<Be<O<N - Atoms with half-filled or completely filled orbitals in the outer shell are more stable and possess higher IE. As atomic radius increases, IE decreases. Although B is smaller than Be, we expect the Be atom to have a higher IE because of the stable 2s2 configuration. N's 1s22s22p3 configuration is more stable than the 1s22s22p4 configuration of O, so N has a greater IE than O. The correct answer choice is B<Be<O<N.

Which of the following species has the largest radius?

Br Br− I I− answer: I- - Iodine is larger than bromine in general, due to an additional shell. Also, the iodide ion is larger than neutral iodine due to the additional electron and the resulting enhanced repulsion.

Which of the following is larger, Br or Br−?

Br- - The larger of the two is Br− because ionic radius increases when you add an electron and decreases when you take one away. This is because electrons repel one another, so adding an electron makes an atom bigger.

C12H22O11 is an example of a(n):

C12H22O11 is an example of a molecular compound - because it consists of two or more elements that are nonmetals, and are covalently bonded.

Which of the following has the lowest electron affinity?

Ca N In Ge answer: Ca - Ca would have the lowest electron affinity because Group 2A has a filled ns subshell. It does not follow the expected trend.

Which of the following isoelectronic particles has the smallest radius?

Ca+2 - Isoelectronic particles all have the same number of electrons but differing number of protons. As the number of protons increases in the series, an increasing nuclear charge is being exerted on the same number of electrons. This means that valence electrons are pulled closer as the number of protons increases. Ca2+ has the greatest number of protons at 20 and will therefore have the smallest radius.

Which of the following is a rule indicated by the Aufbau principle?

Electrons are placed in the lowest energy subshell that is not fully occupied. - The Aufbau principle indicates that electrons are placed in the lowest energy subshell that is not already fully occupied. This order is illustrated by the image below. Different subshells have different capacities and each subshell will be filled before moving on to the next subshell. The s subshells hold 2 electrons. The p subshells hold 6 electrons. The d subshells hold 10 electrons. The f subshells hold 14 electrons.

Elements that have similar electron configurations belong to the same:

Group - Elements in the same group have the same number of valence electrons, so they will be housed in orbitals in a similar way. Thus, they will have similar electron configurations.

Every ________ will have its own unique set of quantum numbers.

Individual electron -Every single electron in an atom will have a unique set of quantum numbers describing its energy and orientation within the atom

Which of the following species is expected to have the smallest radius?

K+ Cl- Ar S2- answer: K+ - These species are isoelectronic, and potassium has the most protons, which means its nucleus exerts the greatest attraction on the electrons.

Which of the following has the highest second ionization energy (IE2)?

Li - The elements listed are all in first group of the periodic table. Ionization energies tend to increase going up a group in the periodic table. Of the elements listed, the element with the largest second ionization energy is lithium because it is the closest to the top of the periodic table.

Of the following choices, the largest decrease in ionic radius occurs when __________.

Na becomes Na+ Na becomes Na+ Ne becomes Ne+ F becomes F+ answer: Na becomes Na+ - When sodium loses its valence electron, it will lose an entire shell, thus dramatically reducing its radius, more so than the other listed elements.

Which of the following species has the largest radius?

O2- F- Ne Na+2 - For any series of isoelectronic particles, the radius decreases as the atomic number (the number of protons) increases. Note that all of these species are isoelectronic with neon, meaning they all have the same number of electrons. Oxygen has the least number of protons of the species listed (smallest atomic number). Therefore, the electrons in O2− will be the least attracted to the nucleus, and so this ion has the largest radius.

The Aufbau principle states that:

Orbitals will be filled in order of increasing energy, which is generally in order of increasing principal quantum number. - It is the Aufbau principle that outlines the precise order in which orbitals will be filled when an atom houses its electrons. The Pauli Exclusion Principal states that no two sets of quantum numbers can be the same. Hund's Rule states that you must place one electron in each orbital in a subshell before doubling up.

Which ion is isoelectronic with krypton?

Rb+ - If rubidium loses its 5s electron it will lose a shell and attain krypton electron configuration.

What is the symbol for the following ion electronic structure: [Ne]3s23p6 with an atomic number of 16?

S^2- - Atomic number 16 corresponds to S but there are 2 more electrons than S usually has so we know that S had to gain (−2).

What is the symbol for the following ion electronic structure: 1s22s22p63s23p63d104s24p64d105s2 with an atomic number of 50?

Sn+2 - Atomic number 50 corresponds to Sn but there are 2 less electrons than Sn usually has (lost electrons = cation) so: Sn+2

Which of the following is NOT a molecular compound?

SnSe2 NH3 PCl5 N2O4 answer: SnSe2

Identify the element with the lowest exothermic (least negative) electron affinity based on periodic trends.

Sr Na F P answer: Sr - Using the periodic table and knowing that the electron affinity generally increases in absolute value (becomes more negative) as we move from left to right and bottom to top, we can determine that Sr would have the lowest (least negative) electron affinity.

The electron affinity (EA) is the energy change for the process of adding an electron to a gaseous atom to form an anion (negative ion). Which of the following is true about the electron affinity?

The sign of the electron affinity depends on the element. - For most elements, the process of adding an electron to a gaseous atom to form an anion (negative ion) is exothermic, which means that energy is released when the gaseous atom accepts an electron. However, for some elements, energy is required for the atom to become negatively charged and the value of their EA is positive.

Electrons that inhabit different orbitals must have a different value for the:

They could have the same principal quantum number if they are in different orbitals with the same shell, they could have the same angular momentum quantum number if they are in different orbitals of the same type of subshell, and they could have the same spin value, as every full orbital will have one electron spin up and one spin down.

in general, covalent bonding can occur between which of the following?

Two neutral atoms - Covalent bonding occurs between two neutral atoms; the electrons are shared between the two atoms so that each can fill its octet.

An increase in the wavelength of electromagnetic radiation is associated with which of the following?

a decrease in frequency - Wavelength and frequency are inversely proportional: As the wavelength increases, the frequency decreases. The inverse proportionality is illustrated in the figure below. This figure also shows the electromagnetic spectrum, the range of all types of electromagnetic radiation.

cation

an atom that has lost electrons - A cation is an atom that has lost electrons and has a positive charge.

The first experimental evidence for the wave-like behavior of electrons supported de Broglie's model by demonstrating:

an interference pattern for electrons reflecting off a crystal - It was an interference pattern for electrons reflecting off a regular atomic pattern in a crystal that demonstrated the wave-like character of electrons, because such a pattern cannot be explained by corpuscular behavior.

The de Broglie expression can be rearranged to give quantization of:

angular momentum - 2πr=nλ=nhp=nhmv=nhrmvr=nhrL This expression can be rearranged to show the formula for the quantinization of angular momentumL=nh2π=nℏ

In German, "aufbau" means:

build up -Aufbau means "build up", which illustrates the meaning of the Aufbau principle, since it tells the order in which we can use orbitals to build up the electron configuration for an atom.

Atoms that form ions with a positive charge are known as __________.

cations - Atoms that form ions with a positive charge are known as cations.

Different ions of a given element will have differing numbers of __________.

electrons - Ions and neutral atoms of the same element differ by having different numbers of electrons.

If the electron affinity for an element is negative, this means that

energy is released when an atom gains an electron. - Electron affinity (EA) is defined as the energy change for the process of adding an electron to a gaseous atom to form an anion (negative ion). Therefore, If the electron affinity for an element is negative, this means that energy is released when an atom gains an electron. In other words, a negative value for the electron affinity means that the process of gaining an electron is exothermic, and is an energetically favorable process.

Deviations to the trends in first ionization energy occur because of which of the following?

increased destabilization from electron repulsion - For example, there is a decrease in ionization energy from nitrogen to oxygen because nitrogen has half-filled p orbitals, while oxygen has an extra electron that must share an orbital with another electron. This additional repulsion destabilizes the electron beyond what is compensated by the increase in Zeff. This increased destabilization results in a decrease in ionization energy.

As we move down the groups of the periodic table (increasing atomic number), cations with the same charge have __________.

larger radii - As we move down the groups of the periodic table, cations with the same charge have larger radii because they have additional shells of electrons.

Which of the following have the last electron added in an s or p orbital?

main group -The main group elements have the last electron added in an s or p orbital. The transition metals and inner transition metals have the last electron added in a d or f orbital, respectively.

If mass and velocity are unknown when using de Broglie's wavelength formula, what alternative value must we have to successfully determine the wavelength?

momentum - de Broglie's wavelength formula is λ=hp or λ=hmv. Therefore if we are unable to determine mass and velocity, we must know the momentum of the particle.

Which of the following labels are used for quantum numbers to describe the state of an electron inside an atom? Select all that apply.

ms 1 The magnetic quantum number (ml), the spin quantum number (ms), the principal quantum number (n), and the angular momentum quantum number (l) all describe electrons within atoms. (m) and (mo) are not labels used to describe the state of an electron in an atom.

Which of the following quantum numbers describes an electron in an atom? Select all that apply.

ms, m1, 1 and n - The magnetic quantum number (ml), the spin quantum number (ms), the principle quantum number (n), and the angular momentum quantum number (l) all describe an electron.

Which set of quantum numbers is invalid?

n=0,l=0,ml=0,ms=1/2 - The principal quantum number, n, must be at least 1.

Which set of quantum numbers is invalid?

n=1, l=1, ml=0, ms=1/2 -The principle quantum number is n. The angular momentum quantum number, l, must be an integer from 0 to n−1, inclusive. The magnetic quantum number, ml, must be an integer between −l and l, inclusive. Therefore, l must be less than n, so the set of quantum numbers, n=1,l=1,ml=0,ms=12, is invalid.

Which set of quantum numbers is invalid?

n=2, l=0, ml=−1, ms=1/2 - Since l =0 indicates a s-orbital (sphere-shaped), there are no additional vector directions and the magnetic quantum number ml must also be zero. Therefore, the option n=2,l=0,ml=−1,ms=12 does not represent a valid set of quantum numbers.

The group that is least likely to ionize is the __________.

noble gases - The noble gases are also called the inert gases because they are very unlikely to react. This is because they have a full valence shell of electrons, which means they do not want to gain or lose any electrons. The other groups listed all readily ionize.

Which of the following pairings usually forms molecular compounds?

nonmetal + nonmetal

For a given energy level, which of the following subshells has the 2nd lowest energy?

p s, p, d, f

The angular momentum of an electron will be:

perpendicular to its orbit - The angular momentum of an object in circular motion, whether an electron or a macroscopic object, will be perpendicular to the plane of circular motion.

Which of the following results in a decrease in Zeff, given that the number of protons remains the same?

the addition of one or more electrons to the valence shell - Zeff is the effective nuclear charge, the charge that leads to the Coulomb force exerted by the nucleus on an electron, calculated as the nuclear charge minus shielding. The addition of one or more electrons to the valence shell with the same number of protons present leads to a decrease in Zeff.

An especially large increase in ionization energy occurs when __________.

the next electron to be removed is a core electron - If the last electron removed is the last of a valence shell, it has suddenly dropped in size significantly and has also attained noble gas electron configuration, and so the next electron to be removed is a core electron rather than a valence electron. Therefore, removing another electron will be particularly energetically unfavorable.

What determines the difference in size of atoms or ions if they are isoelectronic?

the number of protons - The number of protons determines the size of atoms or ions that are isoelectronic. Among a group of isoelectonic species, the one with the least number of protons will be largest, and the one with the most will be smallest.

Generally, on the periodic table, ionization energy increases __________.

up and right - Atomic radius and ionization energy follow opposite trends. Atomic radius increases down and left, while ionization energy increases up and right. As we move to the right on the periodic table, we add protons, which contracts the radius and holds electrons more tightly so they are harder to remove.

The ______ is the distance between two consecutive peaks in a wave.

wavelength