Chem 3.6-4.3

Which of the following sets of quantum numbers could describe an electron in a 4p orbital? Select all that apply. 4, 0, 0 4, 1, 0 4, 2, 0 4, 1, -1 4, 1, +2

4, 1, 0 4, 1, -1

Which of the following statements correctly describe the relationship between the electron configuration of an element and its position on the periodic table? Select all that apply. The highest occupied orbital for a Sr atom is a 4d orbital. Elements that are in the same group will have the same outer electron configuration. The highest occupied orbital for a Se atom is a 4p orbital. The electron configurations of transition metals follow a regular trend associated with their group numbers.

Elements that are in the same group will have the same outer electron configuration. The highest occupied orbital for a Se atom is a 4p orbital.

Which of the following statements correctly describe how an orbital diagram is constructed? Select all that apply. Electrons are placed by filling lower energy levels first. Orbitals may be listed horizontally or vertically. Only the orbitals that actually contain electrons are shown, even for sublevels that have more than one orbital. An individual orbital is represented by a box, circle, or line. Electrons are represented by arrows pointing left or right.

Electrons are placed by filling lower energy levels first. Orbitals may be listed horizontally or vertically. An individual orbital is represented by a box, circle, or line.

Which of the following statements correctly describe the atom in terms of quantum mechanics? Select all that apply. Electrons have certain allowed energy states associated with fixed orbits around the nucleus. An electron may be precisely located within an atom if we know which atomic orbital it is in. Electrons exhibit behavior of both waves and particles. The electron density in the atom can be described by wave functions. Each electron occupies a three-dimensional space near the nucleus. This space is described by a wave function.

Electrons exhibit behavior of both waves and particles. The electron density in the atom can be described by wave functions. Each electron occupies a three-dimensional space near the nucleus. This space is described by a wave function.

Which of the following factors lead to the splitting of energy levels into sublevels in many-electron atoms? Select all that apply. Electron spin Orbital shape Electron repulsions

Orbital shape Electron repulsions

True or false: Bohr's theory explains the line spectrum of hydrogen but cannot explain the spectra of other atoms.

true

A condensed electron configuration includes the element symbol of the _____ gas that is _____ to the relevant element in square brackets, followed by the configuration of the energy level being filled. diatomic; prior noble; prior noble; closest diatomic; closest

noble; prior

Hund's rule states that when a sublevel contains several orbitals of equal energy, _______ electron(s) must be placed in each orbital before electrons are ______

one, paired

Which of the following statements correctly describe p orbitals? Select all that apply. p orbitals always occur in groups of three. A p orbital has its highest electron density at the nucleus. A p orbital has a dumbbell shape with two lobes, one on either side of the nucleus. The p orbitals of a group have different shapes and energies. The p orbitals of a group are perpendicular to each other.

p orbitals always occur in groups of three. A p orbital has a dumbbell shape with two lobes, one on either side of the nucleus. The p orbitals of a group are perpendicular to each other.

The relative energies of the orbitals in the hydrogen atom depend on the value of the ______ quantum number but not on the value of the _____ quantum number. angular momentum; principal principal; angular momentum principal; magnetic angular momentum; magnetic

principal; angular momentum

An orbital with ℓ = 0 is called a(n) _____ type orbital and has a(n) _____ shape. There is always a total of _____ orbital(s) of this type for each principal energy level. s, spherical, 1 p, dumbbell, 3 s, spherical, 3 p, spherical, 3

s, spherical, 1

For many-electron systems each principal energy level is split into ____________ of differing energies. The energy of an orbital in such a system is affected by repulsions between ___________ and by orbital shape.

sublevels, electrons

A p orbital has _____ regions or lobes of high electron probability, on either side of the nucleus. This gives the orbital a(n) _____ shape. 2, figure 8 1, figure 8 1, spherical 2, spherical

2, figure 8

Which of the following correctly defines an atomic orbital in terms of the quantum mechanical model of the atom? A wave function that defines a region of probability of finding an electron of a particular energy A well-defined three-dimensional space occupied by an electron of a particular energy A mathematical function that describes the position of the electron wave in three dimensions A fixed orbit or circular pathway that an electron of a particular energy follows

A mathematical function that describes the position of the electron wave in three dimensions

Which of the following statements correctly describe the Aufbau principle? Select all that apply. One electron is placed in each available orbital before pairing any electrons. According to this principle the electron configuration of any element is determined by building it up in steps. An electron configuration diagram for an element is drawn by placing electrons in the highest occupied energy orbitals first. Electrons are placed successively in orbitals, starting with the lowest energy orbital available.

According to this principle the electron configuration of any element is determined by building it up in steps. Electrons are placed successively in orbitals, starting with the lowest energy orbital available.

Which of the following statements correctly describe how to place electrons in orbitals of the same sublevel? Select all that apply. All unpaired electrons in a sublevel should have parallel spins. A pair of electrons is placed in each orbital until all the orbitals of the sublevel are full. Unpaired electrons should alternate in their spins. One electron must be placed in each orbital of equal (degenerate) energy before electrons are paired up.

All unpaired electrons in a sublevel should have parallel spins. One electron must be placed in each orbital of equal (degenerate) energy before electrons are paired up.

Which of the following statements correctly reflects the most important consequence of Pauli's exclusion principle? An energy level can hold a maximum of two electrons of opposite spin. An atomic orbital can hold a maximum of two electrons as long as they have the same spin. An atomic orbital can hold a maximum of two electrons as long as they have opposite spins. Orbits fill from lower to higher energy levels.

An atomic orbital can hold a maximum of two electrons as long as they have opposite spins.

Which of the following statements correctly describe an s orbital? Select all that apply. An s orbital has a spherical shape. s orbitals always occur in pairs. An s orbital can have an mℓ value = 1. A 2s orbital has two regions of higher electron density.

An s orbital has a spherical shape. A 2s orbital has two regions of higher electron density.

Which of the following statements correctly describe different categories of electrons? Select all that apply. Ca has two valence electrons. Core electrons determine how atoms interact with each other. All elements in group 17 react similarly because they all possess 5 valence electrons. Valence electrons are the outermost electrons of an atom. For main group elements, the group number is also the number of valence electrons.

Ca has two valence electrons. Valence electrons are the outermost electrons of an atom. For main group elements, the group number is also the number of valence electrons.

What characteristics do elements in the same group have in common? Select all that that apply. Main group elements in the same group have the same number of valence electrons. Elements in the same group have similar chemical properties. Elements in the same group have similar physical properties. Elements in the same group have the same electron configuration.

Main group elements in the same group have the same number of valence electrons. Elements in the same group have similar chemical properties.

Which of the following options correctly describes the limitations of the Bohr model of the atom? The Bohr model does not account for the existence of a nucleus. The Bohr model cannot explain how atoms emit or absorb energy. The Bohr model cannot explain the existence of atomic line spectra. The Bohr model cannot account for the behavior of multielectron species.

The Bohr model cannot account for the behavior of multielectron species.

Which of the following options interpret the electron configuration 1s22s22p3 correctly? Select all that apply. The electrons in the 2p orbitals might be spinning either clockwise or counterclockwise. In shorthand notation, sublevels are listed in order of the principal energy levels or shells. The two electrons in the 2s sublevel have opposite spin. There are two electrons in the 1s sublevel. There are three electrons in a 2p orbital.

The electrons in the 2p orbitals might be spinning either clockwise or counterclockwise. The two electrons in the 2s sublevel have opposite spin. There are two electrons in the 1s sublevel.

Which of the following statements correctly describe Mendeleev's original periodic table? Select all that apply. The original periodic table was developed by Dmitri Mendeleev. The original periodic table predicted the properties of elements that were not discovered until later. The original periodic table had 66 elements. The original periodic table had elements arranged by atomic number. The original periodic table arranged elements according to their electron configuration.

The original periodic table was developed by Dmitri Mendeleev. The original periodic table predicted the properties of elements that were not discovered until later. The original periodic table had 66 elements.

Which of the following are closely related to the electron configuration of an element? Select all that apply. The type of ion formed by a given element The identity of an element The chemical behavior of a given element The physical properties of an element

The type of ion formed by a given element The chemical behavior of a given element The physical properties of an element

Hund's rule dictates that when electrons are placed in orbitals of equal energy, one electron must be placed in each orbital before electrons are paired. Why is this important? This arrangement allows electron spin to be random, which is favored. This arrangement allows the electrons to alternate their spins. This arrangement allows the greatest number of electrons with the same spin. This arrangement allows the electrons to spin more freely.

This arrangement allows the greatest number of electrons with the same spin.

Which of the following statements correctly describe d orbitals? Select all that apply. d orbitals always occur in sets of 5. The d orbitals within the same shell may have different energies. The d orbitals within the same shell all have the same shape. d orbitals are only possible for n ≥ 3.

d orbitals always occur in sets of 5. d orbitals are only possible for n ≥ 3.

Atoms in which all electrons are paired are referred to as _____, while atoms with one or more unpaired electrons are referred to as _____. diamagnetic; paramagnetic stable; unstable inert; reactive paramagnetic; diamagnetic unstable; stable

diamagnetic; paramagnetic

Degenerate orbitals are equal to each other in ______. quantum number energy shape electron spin

energy

True or False: The atomic orbital of the quantum mechanical model is very similar to the orbit described by the Bohr model.

false

Elements such as Na and K are in the same __________ on the periodic table. These elements have similar chemical properties because they have the same number of _________ electrons.

group, valence

Hund's rule states the most stable configuration occurs when electrons occupy degenerate orbitals in such a way as to _____ the number of electrons with the same spin. minimize pair up maximize cancel

maximize

In the quantum mechanical model of the atom, an electron is viewed as a particle-wave occupying a three-dimensional space near the nucleus. This space is modeled by the ___________ function (Ψ) in the Schrodinger equation. The different functions of Ψ are also called atomic __________, each with a characteristic energy and distribution of electron density.

wave, orbital