CHEM111 4.1-4.3, 4.4-4.5, 4.6-4.7

halogens -><- All elements in this group have a valence-electron configuration of ns^2np^5. noble gases -><- All elements in this group have a valence-electron configuration of ns^2np^6 transition metals -><- All elements in this group have incompletely filled d subshells lanthanides and actinides -><- All elements in this group have incompletely filled f subshells.

Each of the following groups of elements have similar chemical properties, but for different reasons. Match each group with the correct reason for the similarities within the group. halogens -> noble gases -> transition metals -> lanthanides and actinides -> <- All elements in this group have incompletely filled f subshells. <- All elements in this group have a valence-electron configuration of ns^2np^5. <- All elements in this group have incompletely filled d subshells <- All elements in this group have a valence-electron configuration of ns^2np^6

n -><- Principal energy level or shell of the relevant electrons l -><- Sublevel of the relevant electrons # -><- Number of electrons in the given sublevel.

Electron configuration can be designated using a shorthand notation of the general form nl# (e.g., 1s2). Match each letter and number in the notation with its correct meaning. n -> l -> # -> <- Principal energy level or shell of the relevant electrons <- Number of electrons in the given sublevel. <- Sublevel of the relevant electrons

group valence

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.

- Li - B - N - He

List the following elements in order of decreasing atomic radius (largest at the top to smallest at the bottom). - B - N - He - Li

- Li - B - N - He

List the following elements in order of decreasing atomic radius (largest at the top to smallest at the bottom). - He - B - Li - N

Rb+ Kr Br- Se2-

List the following species in order of increasing size, starting with the atom/ion with the smallest radius on top to the largest at the bottom. Kr Br- Se2- Rb+

- K - Ca - As - Br

Order the following elements in terms of increasing effective nuclear charge (Zeff), starting with the element that has the lowest effective nuclear charge at the top of the list. - As - Br - Ca - K

3p 3s 2p 2s 1s

Place the orbitals in the order that they would be filled according to the Aufbau principle. Place the orbitals lowest in energy at the bottom of the list. 1s 2p 3s 3p 2s

S2- Ca2+ K+ Sc3+

Predict the arrangement of the following isoelectronic ions in increasing size (with the smallest at the bottom). Sc3+ S2- Ca2+ K+

- Mg - Ca

Using the modern periodic table, select the two elements whose chemical properties you would expect to be similar. Multiple select question. - As - Cl - Se - Mg - Ca

- F- - O2- - Na+

Which of the following monatomic ions have the electron configuration 1s22s22p6? Select all that apply. Multiple select question. - Na+ - O2- - Li+ - S2- - F-

- A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. - The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell. - When an atom gains one or more electrons, its radius increases due to electron-electron repulsions.

A cation is smaller than its parent atom, whereas an anion is larger. Which of the following statements correctly explain this observation? Select all that apply. Multiple select question. - A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. - When an anion is formed its radius increases because it gains an electronic energy level. - The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell. - When an atom gains one or more electrons, its radius increases due to electron-electron repulsions.

- noble; prior

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. Multiple choice question. - noble; prior - noble; closest - diatomic; prior - diatomic; closest

- S - Br - Se - I

Arrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list. - Br - S - Se - I

- Rb - K - Ca - Br

Arrange the following elements in order of increasing ionization energies (lowest at the top, highest at the bottom) based on periodic trends. - Ca - Rb - Br - K

H- H+ H

Arrange the following ions in increasing size with the smallest at the bottom. H- H+ H

- increases, core

As we move from left to right in the periodic table the effective nuclear charge (Zeff) _____ because the number of _____ electrons remains the same while the actual nuclear charge increases. Multiple choice question. - decreases, valence - increases, core - increases, valence - decreases, core

- increases, more

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 shell. These additional electrons are not shielded as well by inner electrons and are therefore attracted ______ strongly by the nucleus. Multiple choice question. - increases, more - increases, less - decreases, less - decreases, more

K -><- Cs Mg -><- Sr F -><- Cl Ne -><- Ar

Based on their positions in the periodic table, match the elements that are most chemically similar. K -> Mg -> F -> Ne -> <- Sr <- Cl <- Cs <- Ar

- 3d

For a many-electron atom, which of the following sublevels has the highest energy? Multiple choice question. - 3s - 4s - 3p - 3d

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

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? Multiple choice question. - This arrangement allows the greatest number of electrons with the same spin. - This arrangement allows electron spin to be random, which is favored. - This arrangement allows the electrons to alternate their spins. - This arrangement allows the electrons to spin more freely.

one paired

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 ______.

- maximize

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. Multiple choice question. - maximize - pair up - minimize - cancel

- shielding

In a multi-electron atom, repulsions between electrons prevent valence electrons from "experiencing" the full positive charge of the nucleus. This repulsion is known as ______. Multiple choice question. - shielding - electron affinity - effective nuclear charge - periodicity

- F; S

In each of the following pairs of elements, select the element that will have the greater value for electron affinity.(i) Li vs. F(ii) P vs. S Multiple choice question. - Li; P - F; P - Li; S - F; S

- decrease, increase

In general for main group elements atomic radii _____ from left to right across a period and _____ down a group of the periodic table. Multiple choice question. - decrease, increase - decrease, decrease - increase, decrease - increase, increase

- farther away from; more

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. Multiple choice question. - closer to; more - closer to; less - farther away from; less - farther away from; more

Elements in Groups 1, 2 and 13-17 -><- main group elements Group 18 -><- noble gases Elements in Groups 3-11 -><- transition metals f-block transition elements - ><- lanthanides and actinides

Match each group number from the periodic table with the correct name. Elements in Groups 1, 2 and 13-17 -> Group 18 -> Elements in Groups 3-11 -> f-block transition elements - > <- noble gases <- lanthanides and actinides <- transition metals <- main group elements

completely filled p subshells -><- noble gases (except He) incompletely filled d subshells -><- transition metals incompletely filled f subshells -><- lanthanides and actinides

Match each group of the periodic table with the type of electron configuration exhibited by elements in that group. completely filled p subshells -> incompletely filled d subshells -> incompletely filled f subshells -> <- noble gases (except He) <- transition metals <- lanthanides and actinides

Pd^2+ -><- [Kr]4d^8 Zn^2+ -><- [Ar]3d^10 Ti^2+ -><- [Ar]3d^2 Mn^2+ -><- [Ar]3d^5

Match each monatomic ion with its correct electron configuration. Pd^2+ -> Zn^2+ -> Ti^2+ -> Mn^2+ -> <- [Ar]3d^5 <- [Ar]3d^2 <- [Ar]3d^10 <- [Kr]4d^8

K -><- loses 1 electron Cl -><- gains 1 electron Mg -><- loses 2 electrons S -><- gains 2 electrons ​

Match each of the following elements with the correct number of electrons lost or gained to form its most common ion. K -> Cl -> Mg -> S -> <- gains 1 electron <- gains 2 electrons <- loses 1 electron <- loses 2 electrons

Main group s-block metals -><- lose all electrons from ns sublevel Main group p-block metals -><- lose first the np electrons, then the ns electrons Main group nonmetals -><- gain electrons to fill the np sublevel Transition metals -><- lose ns electrons before losing (n-1)d electrons

Match each type of element with the typical trend it follows when forming an ion. Main group s-block metals -> Main group p-block metals -> Main group nonmetals -> Transition metals -> <- lose first the np electrons, then the ns electrons <- lose ns electrons before losing (n-1)d electrons <- lose all electrons from ns sublevel <- gain electrons to fill the np sublevel

Cation -><- smaller than its parent atom Anion -><- larger than its parent atom

Match each type of ion with the correct description of its size relative to its parent atom. Cation -> Anion -> <- smaller than its parent atom <- larger than its parent atom

IE decreases -><- down a group. IE increases -><- from left to right across a period.

Match the trends in ionization energies correctly. IE decreases -> IE increases -> <- from left to right across a period. <- down a group.

- isoelectronic

Mg2+, Na+, and F- all have the same electron configuration as Ne, and are described as being _____ with Ne and with each other. Multiple choice question. - electron equivalent - isoelectric - pseudo-noble gases - isoelectronic

f d p 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. - p - s - d - f

shielding effective

Repulsions between electrons in a many-electron atom results in a phenomenon known as _____ , which leads to the electrons "experiencing" a lower _____ nuclear charge.

- higher; more; valence

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. Multiple choice question. - lower; less; valence - higher; more; valence - lower; less; core - higher; more; core

- [Ne]3s23p4

Select the correct condensed electron configuration for the element S (Z = 16). Multiple choice question. - [Ne]2s22p4 - [Mg]3p4 - [Ar]3s23p4 - [Ne]3s23p4

- [Kr]4d10 -> Reason: Sn ([Kr]5s24d105p2) loses the two 5s electrons and two 5p electrons to form Sn4+, which has the configuration [Kr]4d10.

Select the correct electron configuration for Sn4+. Multiple choice question. - [Kr]5s24d8 - [Kr]5s24d65p2 - [Kr]4d10 - [Xe]4d10

- Na

Using the modern periodic table, select the element whose chemical properties you would expect to be similar to potassium, K. Multiple choice question. - Ar - Si - Mg - Na

exclusion 2

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 _____.

configuration

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

ionization cation positive

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 a(n) _____ , which is an ion with a net ______ charge.

effective less shield

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.

valence

The outermost electrons of an atom are called _____ electrons.

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

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

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

What does it mean if two species are isoelectronic? Select all that apply. Multiple select question. - They have the same electron configuration. - They have the same number of electrons. - They are in the same group in the periodic table. - They have the same charge.

- electron-electron repulsions

When an electron is removed from an atom the atomic radius decreases and when an electron is added the atomic radius increases. This is due in large part to changes in _____. Multiple choice question. - electron-nucleus attractions - electron-electron repulsions - electron-electron attractions - electron-nucleus repulsions

- lower; first; spin

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 _____. Multiple choice question. - higher; second; charge - lower; first; spin - higher; first; spin - lower; first; charge - lower; second; spin

- 4s

Which electrons are removed first when forming cations of period 4 transition elements? Multiple choice question. - 3d - 3p - 4d - 4s

- 4s

Which electrons are removed first when forming cations of period 4 transition elements? Multiple choice question. - 4d - 4s - 3p - 3d

- Mg

Which element has the ground-state electron configuration 1s22s22p63s2? Multiple choice question. - Be - Na - Mg - Ca

Mg

Which element has the ground-state electron configuration 1s22s22p63s2? Multiple choice question. - Mg - Ca - Na - Be

- Mg

Which element has the lowest second ionization energy? Multiple choice question. - Si - Al - Mg - P

- P

Which element will have similar chemical properties to an element with Z = 7? Multiple choice question. - Rh - O - Cl - P

Mg -><- 3s As -><- 4p Co -><- 3d F -><- 2p

Which is the highest occupied orbital for each of the following elements, based on their position on the periodic table? Mg -> As -> Co -> F -> <- 3d <- 3s <- 4p <- 2p

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

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

- Ne

Which of the following elements is expected to have the highest first ionization energy, based on periodic trends? Multiple choice question. - Ne - Cl - Ca - P

- Cl

Which of the following elements will have the greatest effective nuclear charge? Multiple choice question. - Cl - S - Na - Mg

- Alkali metals - Noble gases - Halogens

Which of the following groups contains elements that are chemically similar to each other because they have the same valence-electron configuration? Select all that apply. Multiple select question. - Alkali metals - Halogens - Transition metals - Noble gases

Cl- K+ S2-

Which of the following ions are isoelectronic with Ar? Select all that apply. K+ S2- Br- Mg2+ Cl-

- 1s22s22p63s23p64s23d104p1

Which of the following is the correct ground-state electron configuration for gallium (Ga; Z = 31)? Multiple choice question. - 1s22s22p63s23p64s24p1 - 1s22s22p63s23p64s23d11 - 1s22s22p63s23p64s23d104p1 - 1s22s22p63s23p64s24d104p1

A

Which of the following is the correct orbital diagram for sulfur (Z = 16)? - A - B - C - D

- Mn4+ [Ar]4d3

Which of the following metal ion electron configurations is incorrect? Multiple choice question. - Ag+ [Kr]4d10 - Fe3+ [Ar]3d5 - Mn4+ [Ar]4d3 - Zr3+ [Kr]4d1 - Cd2+ [Kr]4d10

- Na+ - F- - O2-

Which of the following monatomic ions have the electron configuration 1s22s22p6? Select all that apply. Multiple select question. - Li+ - Na+ - F- - O2- - S2-

- The charge of a main group cation is equal to its group number. - Metals generally form cations. - Noble gases do not usually form ions.

Which of the following options correctly describe the general trends followed by elements when they form ions? Select all that apply. Multiple select question. - Nonmetals tend to lose electrons. - Metals generally form cations. - The charge of a main group cation is equal to its group number. - The charge of a main group anion is equal to (18 - group number). - Noble gases do not usually form ions.

- Inner electrons are more effective at shielding outer electrons than electrons in the same level. - The shielding effect increases with an increasing number of electrons in a given sublevel. - Shielding reduces the magnitude of the nuclear charge a given electron experiences.

Which of the following options correctly describe the shielding effects in a many-electron system? Select all that apply. Multiple select question. - The shielding effect increases with an increasing number of electrons in a given sublevel. - Shielding protects an electron so that it is harder to remove from the atom. - Shielding reduces the magnitude of the nuclear charge a given electron experiences. - Electrons in the same sublevel do not shield each other from the nucleus. - Inner electrons are more effective at shielding outer electrons than electrons in the same level.

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

- Br- - Sr2+

Which of the following species are isoelectronic with each other? Select all that apply. Multiple select question. - Cd2+ - Ar - Br- - Sr2+ - Mg2+

- Atomic radii of main group elements decrease from Group 1A to Group 8A. - Atomic radii generally increase as n increases.

Which of the following statements correctly describe atomic radii? Select all that apply. Multiple select question. - Atomic radii decrease as the effective nuclear charge (Zeff) decreases. - Atomic radii of main group elements decrease from Group 1A to Group 8A. - Atomic radii generally increase as n increases.

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

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

- 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 effective nuclear charge (Zeff)? Select all that apply. Multiple select question. - A lower Zeff is due to the loss of a proton from the nucleus. - Effective nuclear charge is lowered by electron-electron repulsions. - A lower Zeff makes a given electron easier to remove. - Effective nuclear charge is only lowered by inner electrons.

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

Which of the following statements correctly describe electron affinity? Select all that apply. Multiple select question. - Electron affinity measures the tendency of an element to form an anion. - An element with a high electron affinity will not gain an electron easily. - Electron affinity is the energy released during the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions. - Most electron affinities are negative. - The overall trend in electron affinities is to increase from left to right across a period.

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

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

- 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.

Which of the following statements correctly describe how to place electrons in orbitals of the same sublevel? Select all that apply. Multiple select question. - 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. - Unpaired electrons should alternate in their spins. - A pair of electrons is placed in each orbital until all the orbitals of the sublevel are full.

- 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 the Aufbau principle? Select all that apply. Multiple select question. - 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. - 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.

- The number of valence electrons increases for representative elements. - The nuclear charge increases.

Which of the following statements correctly describe the changes that occur as we move from left to right across the periodic table? Select all that apply. Multiple select question. - The nuclear charge felt by the outermost electrons decreases. - The number of core electrons increases. - The number of valence electrons increases for representative elements. - The nuclear charge increases.

- 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 the relationship between the electron configuration of an element and its position on the periodic table? Select all that apply. Multiple select question. - The highest occupied orbital for a Se atom is a 4p orbital. - 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 electron configurations of transition metals follow a regular trend associated with their group numbers.

- Anions are larger than their parent atom. - Ionic size increases down a group on the periodic table.

Which of the following statements correctly describe the trends in ionic size? Select all that apply. Multiple select question. - For cations of the same element, cation size increases with increasing charge. - Ionic size increases down a group on the periodic table. - Cations are smaller than their parent atom because of an increase in electron-electron repulsion. - Anions are larger than their parent atom.

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

Which of the following statements correctly describe the trends in ionization energy (IE)? Select all that apply. Multiple select question. - Noble gases have high ionization energies. - Second ionization energies are always less than first ionization energies. - Atoms with low ionization energies tend to form cations. - Nonmetals tend to have low ionization energies.

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

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

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

Which of the following statements describe/define ionization energy correctly? Select all that apply. Multiple select question. - The ionization energy of an element is a measure of how easily it forms an anion. - The ionization energy of an element is a measure of how easily it forms a cation. - Ionization energy is the energy (kJ) required for the complete removal of 1 mol of valence electrons from 1 mol of gaseous atoms or ions. - Ionization energy is the energy required for complete removal of 1 mol of core electrons from 1 mol of gaseous atoms or ions.

- 2p

Which type of electrons are best at shielding a 3p electron? Multiple choice question. - 4p - 3s - 3d - 3p - 2p

Why does atomic radius generally increase down a group on the periodic table? Multiple choice question. Moving down a group, the outer electrons are at increasingly higher energy levels, causing them to be farther from the nucleus. Electron-electron repulsions become stronger the farther away from the nucleus the electrons are located. The charge on the nucleus decreases and the outer electrons are therefore attracted less strongly.

Why does atomic radius generally increase down a group on the periodic table? Multiple choice question. - Moving down a group, the outer electrons are at increasingly higher energy levels, causing them to be farther from the nucleus. - Electron-electron repulsions become stronger the farther away from the nucleus the electrons are located. - The charge on the nucleus decreases and the outer electrons are therefore attracted less strongly.

- Electron repulsions increase, making it easier to remove the outermost electron.

Why does ionization energy generally increase from left to right across a period? Multiple choice question. - Electron repulsions decrease, making it harder to remove the outermost electron. - The closer one gets to a noble gas the more likely an element is to gain an electron. - Effective nuclear charge increases and the outermost electron becomes harder to remove. - Electron repulsions increase, making it easier to remove the outermost electron.

F F^- O^2- N^3-

Without reference to Figure 4.13, list the following species in order of increasing radius, with the species with the smallest radius at the top of the list. - F - N^3- - F^- - O^2-

15 electrons -><- p-block 20 electrons -><- s-block 43 electrons -><- d-block

Without reference to the periodic table, match each atom (number of electrons given) with its block designation (s-, p-, or d-block) on the periodic table. Hint: Write out the electron configuration for each example. 15 electrons -> 20 electrons -> 43 electrons -> <- s-block <- p-block <- d-block

- [Ar]4s23d104p5 - 1s22s22p63s23p64s23d104p5

Without using the periodic table, which of the following correctly represent the electron configuration of an element with 35 electrons? Select all that apply. Multiple select question. - 1s22s22p63s23p64s23d104p5 - 1s22s22p63s23p5 - 3d104s24p5 - [Ar]4s23d104p5