chem 5

Which of the following options correctly describe the trends in ionization energy (IE)? Select all that apply.

-Atoms with low ionization energies tend to form cations. -Noble gases have high ionization energies.

For a many-electron atom, which of the following sublevels has the highest energy?

3d

Which electrons are removed first when forming cations of Period 4 transition elements?

4s

IE decreases - down a group

IE increases - left to right across a period

For which elements are outer electrons and valence electrons the same?

Main-group elements

Which element has the lowest second ionization energy?

Mg

Why does atomic size generally increase down a group on the periodic table?

The outer electrons are increasingly farther away from the nucleus and shielded more effectively by additional shells of inner electrons.

Which of the following species has a pseudo-noble gas configuration? Select all that apply.

Zn2+ Sn4+

Which of the following is the correct condensed electron configuration for the element S (Z = 16)?

[Ne] 3s23p4

The nuclear charge an electron actually experiences is called the __________ nuclear charge (Zeff). This charge is always _________ than the actual nuclear charge since in a many-electron system the electrons __________ each other from the nucleus.

effective less shield

The first three quantum numbers describe the ________ a particular electron is in whereas the fourth quantum number describes the ____________of an electron.

obital spin

n l ml ms

size shape orientation spin

An electron not only moves around the nucleus but also ______ on its own axis, thus generating a tiny ______ field. The direction of this field is described by the _________quantum number, ms, which is not related to any specific orbital but is a property of the electron itself.

spins magnetic spin

The electron configuration of an element describes _____.

the distribution of electrons in the orbitals of its atoms

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. -One electron must be placed in each orbital of equal (degenerate) energy before electrons are paired up.

Which of the following statements correctly describe the trends in ionic size? Select all that apply.

-Anions are larger than their parent atom. -Ionic size increases down a group on the periodic table. -Within an isoelectronic series, size decreases with increasing nuclear charge.

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. -An individual orbital is represented by a box or line. -Orbitals may be listed horizontally or vertically.

Which of the following statements describe/define ionization energy correctly? Select all that apply.

-Ionization energy is the energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions. -The ionization energy of an element is a measure of how easily it forms a cation.

Which of the following statements correctly describe atomic radii? Select all that apply.

-The atomic radius of main-group elements decreases across a period. -Atomic size does not change consistently within a period for transition metals. -Atomic radii generally increase as n increases.

Which of the following statements correctly describe many-electron atoms? Select all that apply.

-The fourth quantum number becomes important in describing an individual electron. -The energies of the orbitals in the atom are affected both by the nuclear charge and by the presence of other electrons. -Principal energy levels are split into sublevels.

Which of the following statements correctly describe the original periodic table? Select all that apply.

-The original periodic table was developed by Dmitri Mendeleev. -The original periodic table had 65 elements. -The original periodic table predicted the properties of elements that were not discovered until later.

Which of the following options correctly interpret the electron configuration 1s22s22p3? Select all that apply.

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

Which of the following features arise when depicting and populating an orbital energy diagram for a many-electron atom? Select all that apply.

-There is a limit is on the number of electrons in an orbital. -A spin quantum number is assigned to each electron. -Principal energy levels are split into sublevels.

Select all the options that correctly complete the sentence: The ground-state electron configuration _____.

-obeys Hund's rule -obeys the aufbau principle

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 the ______ charge, by repulsions between _______, and by orbital shape.

-sublevels - nuclear - electrons

Which of the following statements correctly describe effective nuclear charge (Zeff)? Select all that apply.

-the effective nuclear charge is lowered by electron-electron repulsions. -a lower Zeff makes a given electron easier to remove.

Which of the following statements correctly describe electron affinity? Select all that apply.

-the electron affinity is the energy change for the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions .-the overall trend in electron affinities is to increase from left to right across a period .-electron affinity measures the tendency of an element to form an anion.

Which of the following statements correctly describe ground-state electron configurations? Select all that apply.

-the ground-state electron configuration has the lowest-energy distribution of the electrons-the ground-state electron configurations are the basis for the recurring pattern of chemical behavior

Which of the following statements correctly reflects the most important consequence of Pauli's exclusion principle?

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

Which of the following atoms has the lowest 1s sublevel energy?

C

______ are smaller than their parent atoms and ______ are larger than their parent atoms.

Cations; anions

Why does ionization energy generally increase from left to right across a period?

Effective nuclear charge increases, and the outermost electron becomes harder to remove.

Electron affinity increases matches Choice, across a period. across a period.

Electron affinity do not change greatly matches Choice, down a group. down a group.

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

Electron repulsions Nuclear attraction Orbital shape

Which of the following options correctly describe metallic behavior? Select all that apply.

High electrical and thermal conductivity A tendency to lose electrons and form cations

1. f 2. d 3. p 4. s

Rank the sublevels for a particular principal energy level in order of decreasing energy for a many-electron atom. Place the lowest energy sublevel at the bottom of the list.

Each electron in a many-electron system _____ other electrons from the nucleus because electron-electron _____ to some extent counteract the nuclear attraction and ______ the energy of an orbital.

Shields, Repulsion, Increases.

Which of the following statements correctly describe the spin quantum number of the electron? Select all that apply.

The spin quantum number has values of +1212 or -1212. The spin quantum number is a property of the electron itself.

What does it mean if two species are isoelectronic? Select all that apply.

They have the same number of electrons. They have the same electron configuration.

Mendeleev's original 1870 periodic table illustrated that similar chemical and physical properties recur periodically when the 65 known elements at the time were arranged by ______.

atomic mass

The electron ______ of an element shows the distribution of electrons within the electronic energy levels of the atom.

configuration

In general for main-group elements, atomic size _____ from left to right across a period and _____ down a group.

decreases; increases

A species that is slightly repelled by a magnetic field is called ______ and has no unpaired electrons.A species that is attracted to a magnetic field is called ______ and has one or more unpaired electrons.

diamagnetic; paramagnetic

outer elcetrons

electrons in the highest energy level that has electrons

core electrons

electrons in the previous noble gass and any filled d of f sublevels

valence electrons

eletrons involoed in bonding

The Pauli __________ principle guarantees that no two electrons in the same atom have the same quantum number description. This means that the maximum number of electrons that can be accommodated by any orbital is ___________ .

exclusion two

Ionization energy generally decreases down a group because as one moves down a group, the outermost electron moves _____ the nucleus and it takes _____ energy to remove it.

farther away from; less

Second ionization energies are always _____ than first ionization energies because the remaining electrons are attracted _____ strongly as the positive charge on the ion increases. A large jump in ionization energies is always observed after the _____ electrons have been removed.

higher; more; valence

As we move down a group in the periodic table, both atomic and ionic radii tend to _____. Comparisons of ionic radii between groups can only be made if the species are isoelectronic. For an isoelectronic series of ions, cations are _____ than anions.

increase, smaller

Metallic behavior tends to _____ down a group in the periodic table and _____ from left to right across a period.

increase; decrease

For electronic sublevels within the same principal energy level, in general a higher nuclear charge _____ nucleus-electron attractions and therefore _____ sublevel energies.

increases decreases

Ionization energy (IE) ______ from left to right across the periodic table. The magnitude of the electron affinity (EA) ______ from left to right across the periodic table with a number of exceptions.

increases; increases

Atomic radius generally decreases from left to right across a period because the effective nuclear charge _____ while electrons are being added to the same outer level. These additional electrons are shielded _____ by inner electrons and are therefore attracted _____ strongly by the nucleus.

increases; less well; more

The energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions is called ____________energy. For a neutral element this energy is a measure of how easily the element forms an ion with a __________charge.

ionization positive

Mg2+, Na+, and F- all have the same electron configuration as Ne, and are described as being _____ with Ne and with each other.

isoelectronic

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

Noble gas configuration matches Choice, 1s22s22p63s23p6 1s22s22p63s23p6 Pseudo-noble gas configuration matches Choice, 1s22s22p63s23p63d10 1s22s22p63s23p63d10 Inert pair configuration matches Choice, 1s22s22p63s23p63d104s2 1s22s22p63s23p63d104s2

matching

Noble gases High ionization energy and low electron affinity Nonmetals High ionization energy and high electron affinity metals low ionizations energy and low electron affinity

matchings

Main-group s-block metals matches Choice, Lose all electrons from ns sublevel Lose all electrons from ns sublevel Main-group p-block metals matches Choice, Lose first the np electrons, then the ns electrons Lose first the np electrons, then the ns electrons Main-group nonmetals matches Choice, Gain electrons to fill the np sublevel Gain electrons to fill the np sublevel Transition metals matches Choice, Lose ns electrons before losing (n-1)d electrons Lose ns electrons before losing (n - 1)d electrons

mathcies

A diamagnetic species has matches Choice, no unpaired electrons. no unpaired electrons. A paramagnetic species has matches Choice, one or more unpaired electrons. one or more unpaired electrons. A species that is slightly repelled by a magnetic field is matches Choice, diamagnetic. diamagnetic. A species that is attracted to a magnetic field is matches Choice, paramagnetic. paramagnetic.

mathcing

The spin quantum number is represented by the symbol ______ and has the possible values ______, corresponding to the two directions of the electron's magnetic field.

ms +/- 1/2

The spin quantum number has two possible values. Select them below.

ms = -1/2 ms = +1/2

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.

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

n l #

principal energy lvl sublevel of relevant electrons #of electrons in the given sublevel

Electron-electron repulsions result in each electron _____.

shielding the other electrons from the nucleus