General Chemistry Chapter 8

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

4s

which orbitals are the last to be filled in the actinide series

5f

Match each type of oxide to correctly with its acid-base behavior.

Nonmetal oxides - are acidic Metal oxides - are basic Oxides of metalloids - are amphoteric

an electron with a low ionization energy is more likely to form ____ during reactions, while elements with a high ionization energies tend to form ____. Noble gases are excluded from this trend.

cations; anions

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

they have the same outer electron configuration

match each quantum number with the parameter it describes

n - size (energy) of orbital l - shape of orbital m(l) - orientation of orbital m(s) - spin of electron

Electron configuration can be designated using a shorthand notation using the general form nl^# (e.g. 1s^2). Match each letter to the number in the notation with its correct meaning

n - Principal energy level or shell of the relevant electrons l - sublevel of the relevant electrons # - number of electrons in the given sublevel

Hund's rule states that a sublevel contains several orbits of equal energy, ___ electron(s) must be placed in each orbital before electrons are ___.

one, paired

The first five quantum numbers describe the ____ a particular electron is in whereas the number describes the ____ of the electron.

orbital, spin

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

The electron configuration of an element describes

the distribution of electrons in the orbitals of its atoms

Which sub levels may be utilized in constructing a partial orbital diagram for a period 3 element? select all that apply

- 3p - 3s

An atom of Sn (Z=50) has ____ inner (core) electrons, ____outer electrons, and ____valence electrons

- 4 outer electrons - 46 core electrons - 4 valence electrons

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

- The spin quantum number is a property of the electron itself - The spin quantum number has values of +1/2 or -1/2

Which of the following statements correctly describe general trends in electron configurations? select all that apply.

- for any principal energy level (n), the total number of orbitals possible for that level is equal to n^2 - the period number of an element corresponds to the n value of the highest energy level containing electrons - among main group elements, the outer electron configurations within a group are identical

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 charge consistently within a period for transition metals -atomic radii generally increase as n increases

Which of the following ions are isoelectronic with Ar? Select all that apply.

-S^2- -Cl- -K+

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

-Zn^2+ -Sn^4+

select all the options that correctly complete the sentence. The ground-state electron configuration___.

-obeys Hund's rule -obeys the Aufbau principle

Which of the following options correctly describe the order in which sub levels (designated by nl) are most commonly filled with electrons? select all that apply. (ignore anomalous electron configurations)

-the 3d orbitals are generally filled after the 4s orbitals -the 1s sub level must be filled before electrons are places in the 2s orbital

Using the periodic table, place the sub levels 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

List the following elements in order of decreasing atomic size, starting with the largest at the top

1. Li 2. B 3. N 4. He

Arrange the following elements in order of increasing ionization energies (IE) based on periodic trends, starting with the element that has the LOWEST IE a the TOP of the list

1. Rb 2. K 3. Ca 4. Br

arrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list

1. S 2. Br 3. Se 4. I

Rank the sub levels for a particular energy level in order of decreasing energy for a many-electron atom. Place the LOWEST energy sublevel at the BOTTOM of the list

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

Which type of electrons are best at shielding a 3p electron

2p

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

An atomic orbital can hold a maximum of two electrons as long as they have the SAME SPIN

Match the element with the correct description of its properties or behavior, based on periodiotic trends

C - forms acidic oxides Sb - the Mose metallic metalloid in its group Ba - Most readily forms a cation F -most readily gains electrons

match each category of electron with the correct description

Core electrons - electrons in the previous noble gas and any filled d or f sublevels Outer electrons - electrons in the highest energy level that contains electrons Valence electrons - electrons involved in bonding

Match the trends in ionization energy correctly

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

Match each chemical behavior to the correct description of an element's ionization energy. Noble gases are not included in these description.

Low ionization energy - good reducing agent - forms cations readily - is easily oxidized High ionization energy - tends to be reduced - tends to form anions - good oxidizing agent

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

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

Match each electron configuration to the correct description. Assume that all configurations represent ions

Noble gas configuration - 1s^2, 2s^2, 2p^6, 3s^2, 3p^6 Pseudo-noble gas configuration - 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^10 Inert pair configuration - 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^10, 4s^2

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 m(s), which is not related to any specific orbital but is a property of the electron itself.

Rotates, magnetic, spin

What is the correct ground-state electron configuration for Mo (Z=42)?

[Kr] 5s^1 4d^5

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

decreases; increases

the nuclear charge an electron actually experiences is called the ____ nuclear charge (Z eff). 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 lowest-energy distribution of electrons in the sub levels for an atom of a particular element is called the ____ state electron configuration for that element. This is a close relationship between this distribution and the position of the element on the ___ table, since electron configuration determines both the chemical and physical ____ of an element

ground, periodic, properties

elements that are in the same ___ of the periodic table will have the same___electron configuration and will have very similar chemical___.

group; outer; properties

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 therefore attracted _____ strongly by the nucleus.

increases; less well; more

the energy required to complete removal of 1 mol of electrons from one mol go 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

Mg^2+, Na^+, and F^- all have the same electron configuration as Ne, and are described as being ____ with each other

isoelectronic