CHE 101 Chapter 1 and 2

What is the maximum number of electrons that can occupy a 2p orbital?

two

Moving from left to right across a row of the periodic table, the positive charge of the nucleus _____, causing the ______ electrons to be pulled closer to the nucleus.

increase, valence

What is the electron configuration for neon?

1s2 2s2 2p6

Fill in the blank question. The greater the principal quantum number, the _________ the size of an atomic orbital in a given subshell.

larger

Rank the the elements below in order of increasing atomic size, with the smallest element at the top.

P, Al,Mg,Sr, Ba

Within a period (row) of the periodic table, elements on the left side will be ______ in atomic size than elements on the right side.

larger

According to the Pauli exclusion principle, two electrons in an atomic orbital must have _______ spins.

paired

Rank the atomic orbitals below by size, with the largest on top.

1. 3s 2. 2s 3. 1s

Which of the following are NOT proper shell/subshell designations for atomic orbitals? Select all that apply. Multiple select question. 1p 4f 2f 2d 5p 2s

1p 2f 2d

Which of the following are NOT proper shell/subshell designations for atomic orbitals? Select all that apply. Multiple select question. 2d 2f 4f 5p 2s 1p

2d 2f 1p

elements below in order of decreasing atomic size, with the largest element at the top.

As, Se, Br, Cl, F

The periodic table can be divided into "blocks," which correspond to the sublevel that is filled last when the electron configurations are written for elements in that block. In the diagram shown, the blue squares (A) correspond to the _______ block, the green squares (B) represent the _________ block, and the yellow squares (C) comprise the ________ block.

Blank 1: s Blank 2: d Blank 3: p

Select the two elements that have the same number of dots in their Lewis dot symbols. Multiple select question. Cl C Pb P

C Pb

Why do fireworks containing different metals burn with different colors?

Each metal has a unique line emission spectrum that appears as a different color, when the metal is burned.

For which property of an atomic orbital would the designations s, p, d, or f be used?

Energy subshell

Rank the the elements below in order of increasing atomic size, with the smallest element at the top.

Ne, C, B, Al, In

Rank the the elements below in order of increasing energy to remove an electron, with the lowest energy at the top.

Rb, K, Na, Li, B

What is the electron configuration of an atom?

The arrangement of electrons in the atom's orbitals

What is ionization energy?

The energy required to remove an electron from an atom

According to the quantum mechanical model, what does an atomic orbital tell you about an electron in an atom?

The probability of finding it at a given location

What is the correct condensed ground state electron configuration of sulfur?

[Ne] 3s2 3p4

In populating atomic orbitals with electrons, a 4d orbital will be filled ______ a 5s orbital.

after

A(n) ______ is a probability density map that describes the likelihood of finding an electron in a particular region of an atom.

atomic orbital

When drawing an orbital diagram, orbitals of _____ energy are filled first. By convention, the _____ electron in a given orbital is designated as ↑ and the direction of the arrow indicates the electron _____.

lower; first; spin

When populating an orbital diagram, electrons will occupy the ________ energy orbital(s) available.

lowest

In the Bohr model of the hydrogen atom, an electron can only reside in certain ______ that are at ______ energy levels.

orbits; fixed

The line spectra associated with excited atoms result from the fact that the energy of electromagnetic radiation is ______.

quantized

The electrons with the highest principal quantum number in a main-group atom are known as ______ electrons.

valence

Which of the following statements correctly describe atomic line spectra? Select all that apply. Multiple select question. -An atomic line spectrum arises from the emission of light of specific wavelengths. -Atomic line spectra include radiation outside the visible range of the electromagnetic spectrum. -An atom emits radiation continuously to produce a line spectrum. -Each element has its own unique atomic line spectrum. -An atom emits radiation that contains all wavelengths of the elcetromagnetic system

-An atomic line spectrum arises from the emission of light of specific wavelengths. -Atomic line spectra include radiation outside the visible range of the electromagnetic spectrum. -Each element has its own unique atomic line spectrum.

Which of the following statements correctly represent the Bohr model of the atom? Select all that apply. Multiple select question. -Emission of photons results from the collision of electrons at the same energy level. -An electron can move between orbits if it absorbs a sufficient amount of energy. -When an atom absorbs energy, it causes the electrons to orbit more rapidly. -Electrons circle the nucleus of the atom in fixed orbits.

-An electron can move between orbits if it absorbs a sufficient amount of energy. -Electrons circle the nucleus of the atom in fixed orbits.

Which of the following statements concerning the line spectra of elements are correct? Multiple select question. -Atoms of a given element can only emit certain quantities of photons. -The lines in a spectrum correspond to photons with allowed energies. -A change in the energy absorbed by an atom will result in a different emissions spectrum for an element. -Atoms of a given element can only emit photons of certain energies. -Photon emissions correspond to electron transitions between allowed energy levels.

-The lines in a spectrum correspond to photons with allowed energies. -Atoms of a given element can only emit photons of certain energies. -Photon emissions correspond to electron transitions between allowed energy levels.

What is the electron configuration for beryllium?

1s2 2s2

Which of the following are correct designations for 3d orbitals, with regard to their orientation in space? Select all that apply. Multiple select question. 3dx2 3dz2 3dxyz 3dyz 3dxy

3dz2 3dyz 3dxy

correct valence electron configuration for chlorine?

3s2 3p5

what are possible values for a principal energy level (n)?

4 1 3

Rank the orbitals below in order of decreasing energy, with the highest energy orbital at the top of the list.

4d, 5s, 4p, 4s, 3s

Which of the following is the correct valence electron configuration for arsenic?

4s2 4p3

Which of the following statements are true about information obtained from quantum mechanics? Select all that apply. Multiple select question. Quantum mechanics allows us to map the coordinates of electrons in an atom. An atomic orbital is a probability map describing the likelihood of finding an electron in a particular region of an atom. Quantum mechanics allows us to calculate the probability of finding an electron in a certain region around the nucleus. Probability density maps show the exact locations for an electron.

An atomic orbital is a probability map describing the likelihood of finding an electron in a particular region of an atom. Quantum mechanics allows us to calculate the probability of finding an electron in a certain region around the nucleus.

Which statements about orbital diagrams are correct? Multiple select question. An electron in an orbital is indicated by an arrow. Orbitals are indicated by boxes. An orbital can have any number of electrons, as long as the spins alternate. All of the electrons in an orbital must have the same spin.

An electron in an orbital is indicated by an arrow. Orbitals are indicated by boxes.

Which of the following statements about electron transitions in the Bohr atom and energy emissions/absorptions are correct? Select all that apply. Multiple select question. An electron transition from n = 6 to n = 4 results from the absorption of energy. An electron transition from n = 1 to n = 3 results in the emission of a photon. An electron transition from n = 3 to n = 2 results in the emission of a photon. An electron transition from n = 2 to n = 5 results from the absorption of energy.

An electron transition from n = 3 to n = 2 results in the emission of a photon. An electron transition from n = 2 to n = 5 results from the absorption of energy.

Which statements about s orbitals are correct?

An s orbital is spherically shaped. A 3s orbital is larger than a 1s orbital.

Which statements about s orbitals are correct? Multiple select question. An s orbital is spherically shaped. A 3s orbital is larger than a 1s orbital. A 3s orbital is larger than a 4s orbital. An s orbital is dumbbell-shaped.

An s orbital is spherically shaped. A 3s orbital is larger than a 1s orbital.

Which of the following species have the electron configuration 1s2 2s2 2p6 3s2 3p6?

Ar Cl-- Ca2+

Rank the the elements below in order of increasing metallic character, with the least metallic element at the top.

Ar, S, Si, Sn, Pb

Predict the correct charge on the common ion formed based on the concept of being isoelectronic to noble gas formation.

Br- O2-

Which of the following are steps in drawing a proper Lewis dot symbol for a main-group element? Multiple select question. Pair up as many electrons as possible. Count the total number of electrons. Draw electrons as dots around the elemental symbol. Determine the number of valence electrons.

Draw electrons as dots around the elemental symbol. Determine the number of valence electrons.

Which statement is true about electron orbits in the Bohr model of the hydrogen atom?

Each orbit corresponds to a fixed energy level.

Which of the following are likely to have similar chemical properties? Multiple select question. Elements in the same group of the periodic table Elements with the same noble gas core Elements with the same number of valence electrons Elements with similar atomic masses

Elements in the same group of the periodic table Elements with the same number of valence electrons

Which statements about groups, Lewis dot symbols, and valence electrons are correct? Multiple select question. Elements with the same number of dots in their symbols have similar chemical properties. Elements in the same group have the same number of valence electrons. Elements in the same group will have identical Lewis dot symbols. Elements in the same group will have the same number of dots in their symbols.

Elements with the same number of dots in their symbols have similar chemical properties. Elements in the same group have the same number of valence electrons. Elements in the same group will have the same number of dots in their symbols.

When completing an orbital diagram, all orbitals that are equal in energy are populated with single electrons before there is any pairing. This is a statement of ______.

Hund's rule

Which of the following statements are true about information obtained from quantum mechanics? Select all that apply. Multiple select question. Quantum mechanics allows us to calculate the probability of finding an electron in a certain region around the nucleus. An atomic orbital is a probability map describing the likelihood of finding an electron in a particular region of an atom. Probability density maps show the exact locations for an electron. Quantum mechanics allows us to map the coordinates of electrons in an atom.

Quantum mechanics allows us to calculate the probability of finding an electron in a certain region around the nucleus. An atomic orbital is a probability map describing the likelihood of finding an electron in a particular region of an atom.

Which of the following statements about subshell energies are correct? Multiple select question. The 3s subshell is lower in energy than the 2p subshell. The 3p subshell is higher in energy than the 3d subshell. The 3p subshell is higher in energy than the 2p subshell. The 4s subshell is lower in energy than the 3d subshell. The 4f subshell is higher in energy than the 4d subshell.

The 3p subshell is higher in energy than the 2p subshell. The 4s subshell is lower in energy than the 3d subshell. The 4f subshell is higher in energy than the 4d subshell.

Why are there safety concerns about some inexpensive laser pointers?

The eye's blink mechanism cannot detect retina-damaging infrared radiation.

Which of the following statements are correct regarding the energy required to remove an electron from a main group element? Select all that apply. Multiple select question. The farther an electron is from the nucleus, the easier it is to remove. Valence electrons get farther from the nucleus as you move down a group in the periodic table. The energy to remove an electron from an atom decreases as you move down a group in the periodic table. Valence electrons get closer to the nucleus as you move down a group in the periodic table. The energy to remove an electron from an atom increases as you move down a group in the periodic table. The closer an electron is to the nucleus, the easier it is to remove.

The farther an electron is from the nucleus, the easier it is to remove. Valence electrons get farther from the nucleus as you move down a group in the periodic table. The energy to remove an electron from an atom decreases as you move down a group in the periodic table.

Select the reasons the concurrent 1064-nm beam is potentially more dangerous than the green 532-nm beam in a green-light pointer. Select all that apply. The higher-energy beam penetrates the eyelid and damages the retina. The lower-energy beam does not trigger the protective blink response. The lower-energy beam can pass through the eye and damage the retina. The infrared filter is easy to remove. The higher-energy beam can pass through the eye and damage the retina.

The lower-energy beam does not trigger the protective blink response. The lower-energy beam can pass through the eye and damage the retina. The infrared filter is easy to remove.

Which statements about valence electrons are correct? Multiple select question. Valence electrons consist of the noble gas core of electrons. The outermost electrons of a main group element are the valence electrons. Elements with the same number of valence electrons have similar chemical properties. Valence electrons are responsible for the chemical properties of elements.

The outermost electrons of a main group element are the valence electrons. Elements with the same number of valence electrons have similar chemical properties. Valence electrons are responsible for the chemical properties of elements.

Which statements correctly describe information conveyed in the electron configuration notation 1s2 2s2 2p3? Multiple select question. There are electrons in orbitals at the n = 2 and n = 3 levels. There are electrons in p and s subshells. There are electrons in orbitals at the n = 1 and n = 2 levels. The atom contains a total of 12 electrons.

There are electrons in p and s subshells. There are electrons in orbitals at the n = 1 and n = 2 levels.

Why does atomic size decrease from left to right across a row of the periodic table?

There is an increasing attraction between the nucleus and the valence electrons, pulling them closer.

What is the maximum number of electrons that can be contained in the 1s sublevel?

Two

Which statements are correct regarding the energy required to remove an electron from an atom of the main-group elements?

Valence electrons get closer to the nucleus as you move from left to right across a row of the periodic table. The farther an electron is from the nucleus, the easier it is to remove. The required energies increase as you move from left to right across a row of the periodic table.

formation of ions are correct?

When an atom loses electrons, it becomes positively charged. When an atom gains electrons, it becomes negatively charged. Gain of electrons by an atom results in formation of an anion. Loss of electrons by an atom results in formation of a cation.

Which statements are true about atomic orbitals? Multiple select question. Within a principal energy level, there are energy sublevels. Each sublevel contains a fixed number of orbitals. The number of orbitals at a given principal energy level is not predictable. An atomic orbital is described by a principal energy level n. There is one atomic orbital for every value of n.

Within a principal energy level, there are energy sublevels. Each sublevel contains a fixed number of orbitals. An atomic orbital is described by a principal energy level n.

Fireworks displays result from burning metals that emit one dominant ________ as revealed in their visible line spectra.

color

In Bohr's model of the atom, the quantum number n is associated with the _____ of an electron orbit. The lower the n value, the _____ the electron is to/from the nucleus and the _____ the energy level.

energy, closer, lower

An atomic orbital in the quantum mechanical model can be described by a principal _____ level, similar to the Bohr model. Each of these levels can contain one or more energy _____

energy, subshells

True or false: A 3d orbital can contain a maximum of ten electrons.

false

In the Bohr model of the hydrogen atom, the greater the value of the quantum number n, the ______ the energy of the electron and the ______ its orbit to/from the nucleus.

greater; farther

Absorption of a photon of appropriate energy by a Bohr hydrogen atom results in the electron moving to an orbit of _________ energy. Emission of a photon results in the electron moving to an orbit of __________ energy.

higher, lower

Moving from left to right across a row of the periodic table, the positive charge of the nucleus ______, causing the valence electrons to move ______ the nucleus.

increases; closer to

Which of the following statements correctly describe the principal quantum number n? Select all that apply. Multiple select question. -n can have any positive whole-number value. -The value of n determines the shape of an orbital. -The higher the value of n, the lower the energy level. -The lower the value of n, the greater the probability that the electron is closer to the nucleus.

n can have any positive whole-number value. The lower the value of n, the greater the probability that the electron is closer to the nucleus.

Which statements correctly describe the quantum number n with reference to the Bohr model of the hydrogen atom? -n indicates the energy level of an electron in the atom. -The higher the value of n, the closer the electron is to the center of the atom. -n can have any positive, whole-number value. -n is a measure of the difference in energy between two energy levels. -An electron with n = 2 is at higher energy than an electron with n = 1.

n indicates the energy level of an electron in the atom. n can have any positive, whole-number value. An electron with n = 2 is at higher energy than an electron with n = 1.

In the quantum mechanical model of the atom, an s subshell can contain __________ orbital(s), whereas a d subshell can contain _______ orbital(s).

one, five

Niels Bohr postulated that the electron in a hydrogen atom can occupy any of a series of fixed circular paths, known as_______ . Each of these is characterized by a fixed ________ level.

orbits, energy

Order the subshells of a principal energy level by their energies, with the lowest-energy subshell at the top of the list.

s, p, d, f

True or false: When drawing a Lewis dot symbol, single electrons (dots) should be placed at every position around the symbol (left, right, top, bottom) before any are paired.

true

The maximum number of electrons that can occupy any orbital is _______, Correct Unavailable, and their spins must be _____

two, paired