chapter 8 Gen Chem

Using the periodic table, place the sublevels in the correct order for placing electrons. Start with the first sublevel to be filled at the bottom of the list.

1. 4p 2. 3d 3. 4s 4. 3p 5. 3s

Which of the following options is an acceptable electron configuration for hydrogen?

1s1

Quantum Numbers: numbers, shape,spin, & origentaion

n= Positive whole number, how far from nucleus, tells us energy LevelL= zero:#, tells us shape of orbitalmsubL= -L:L, describes the orientation of orbitals

In the Period 6 inner transition element series, the 4f orbitals begin to be filled after the element _____.

La

Which sublevels may be utilized in constructing a partial orbital diagram for a Period 3 element?

3p 3s

Which sublevels may be utilized in constructing a partial orbital diagram for a Period 3 element? Select all that apply.

3p 3s

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

4s

Which orbitals are the last orbitals being filled in the actinide series?

5f

Which of the following is the correct orbital diagram for the ground state of carbon?

A

Periodic Trends

Across the periods- atomic radius decreases- ionization energy increases- electronegativity increases- effective nuclear charge increaseDown the periods- atomic radius increases- ionization energy decreases- electronegativity decreases- effective nuclear charge decrease

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.

Afbau Principle

An electron occupies the lowest-energy orbital that can receive it

paramagnetic

Atom or substance containing unpaired electrons and is consequently attracted by a magnet.

Which of the following is an acceptable orbital diagram for hydrogen, based on normal conventions?

B

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________

Blank 1: exclusion Blank 2: 2, two, two of opposite spin

Elements that are in the same_______of the periodic table will have the same______electron configuration and will have very similar chemical

Blank 1: group or family Blank 2: outer, valence, valence shell, outermost, or outer shell Blank 3: behavior, properties

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.

Blank 1: ionization or ionisation Blank 2: positive,

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.

Blank 1: spins, rotates, or revolves Blank 2: magnetic Blank 3: spin, electron spin, fourth, 4th

Which of the following species are isoelectronic with each other?

Br-:Reason: Br- and Sr2+ are both isoelectronic with Kr. They are therefore isoelectronic with each other. Sr2+:Reason: Br- and Sr2+ are both isoelectronic with Kr. They are therefore isoelectronic with each other.

Match each element with the correct description of its properties or behavior, based on periodic trends.

C Forms acidic oxides Sb: The most metallic metalloid in its group Ba: Most readily forms a cation F: Most readily gains electrons

electron affinity

Change in energy of a neautral atom when an electrong is added and forms an ion the energy change that occurs when 1 mol of an electron is acquired by a neutral atom Electron affinity increases: across a period Electron affinity do not change greatly matches: down a group.

total electrons-valence electrons

Core electrons

Which of the following ions are isoelectronic with Ar?

K+ S2- Cl-

Match each type of element with the typical trend it follows when forming an ion.

Main-group s-block metals matches: Lose all electrons from ns sublevel Main-group p-block metals matches: 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

Which element has the ground-state electron configuration 1s22s22p3?

N

Which of the following monatomic ions have the electron configuration 1s22s22p6?

Na+ O2- F-

Match each electron configuration to the correct description

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

effective nuclear charge

Overall attraction that e⁻ experiences from the nucleus

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

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

Which of the following statements correctly describe many-electron atoms?

Principal energy levels are split into sublevels. 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.

Which of the following options correctly describe the order in which sublevels (designated by nl) are most commonly filled with electrons?

The 3d orbitals are generally filled after the 4s orbital. The 1s sublevel must be filled before electrons are placed in the 2s orbital.

ionization energy

The amount of energy required to lose 1 mol of the valence electrons

Which of the following statements correctly describe atomic radii?

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

Electronegativity

The capacity of the nucleus of an atom to attract a pair of electrons in a covalent bond

core electrons

The electrons in the inner shells of an atom; these electrons are not involved in forming bonds.

Which of the following statements correctly describe ground-state electron configurations?

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

Which of the following statements describe/define ionization energy correctly?

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

Which of the following statements correctly describe electron affinity?

The overall trend in electron affinities is to increase from left to right across a period. The electron affinity is the energy change for 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 the spin quantum number of the electron?

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?

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

Which of the following accounts for the observation that Li, Na, K, and Cs have similar chemical properties?

They have the same outer electron configuration.

Which of the following statements correctly describes a partial orbital diagram?

This diagram includes only the orbitals containing the outer and/or valence electrons of the element.

Which of the following species has a pseudo-noble gas configuration?

Zn2+:Reason: If Zn (Z = 30) loses two e-, it will have the same configuration as Ar with a full 3d sublevel added. Sn4+:Reason: If Sn (Z = 50) loses 4e-, it will have the same configuration as Kr with a full 4d sublevel added

Which of the following is the correct condensed electron configuration for selenium (Z = 34)?

[Ar] 4s23d104p4

Which of the following is the correct condensed electron configuration for titanium (Z = 22)?

[Ar] 4s23d2

Which of the following options gives the correct electron configuration for Sn4+?

[Kr] 4d10 Reason: Sn has a ground-state electron configuration of [Kr] 5s24d105p2. Sn loses the 5s and 5p electrons to form Sn4+.

diamagnetic

all electrons are paired

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

The energy involved in adding 1 mol of electrons to 1 mol of gaseous atoms or ions is called_______Its periodic trends show many variations.

electron affinity

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

isoelectronic

how many valence electrons

number of electrons in the last energy level

The ground-state electron configuration _____.

obeys the aufbau principle obeys Hund's rule

Hund's Rule

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

Isoelectronic

same electron configuration as another element

Paulie Exclusion Principle

states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins

atomic radius

the approximate distance from the nucleus of an atom to its valence electrons

The electron configuration of an element describes _____.

the distribution of electrons in the orbitals of its atoms

groundstate

the lowest allowable energy state of an atom

Zeff (effective nuclear charge)

the positive charge/attraction of the nucleus experienced by the valence electrons (increases moving across the periodic table w/ increased # of protons -- makes the atom smaller because the force holds it tight)