Chem... CH. 3 Hw b

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as

Hunds rule

Which of the following elements is a halogen?

I

Choose the orbital diagram that represents the ground state of N.

1s:^> 2s:^> 2p:^^^; >=down arrow; Nitrogen has atomic # of 7

Give the complete electronic configuration for Mn.

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5

Predict the charge that an aluminum ion would have

3+ look @ #52

Choose the valence orbital diagram that represents the ground state of Zn.

4s:^>(4s^2) 3d:^> ^> ^> ^> ^> (3d^10)

In the ground-state electron configuration of Fe3+, how many unpaired electrons are present?

5

Give a combination of four quantum numbers that could be assigned to an electron occupying a 5p orbital.

5,1,-1, 1/2

Give a combination of four quantum numbers that could be assigned to an electron occupying a 6d orbital.

6,2,-2,-1/2

How many valence electrons do the noble gases possess?

8 VE

Choose the ground state electron configuration for Cr3+.

[Ar]4d2 3d4 ---> [Ar]3d3

Choose the ground state electron configuration for Ti2+.

[Ar]4s2 3d2 ---> [ar]3d2

What is electron affinity?

energy change associated with the gaining of an electron by the atom in the gaseous state

Give the complete electronic configuration for Ca2+.

1s22s22p63s23p6

What is the electron configuration of calcium, which has 20 electrons?

[Ar]4s2

Give the ground state electron configuration for Se.

[Ar]4s^2 3d^10 4p^4 LOOK @ PERIODIC

Give the ground state electron configuration for Sr.

[Kr]5s2

Give the ground state electron configuration for I.

[Kr]5s^2 4d^10 5p^5

Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. P Ge Zr I

[Ne]3s^23p^3 [Ar]4s^23d^104p^2 [Kr]5s^24d^2 [Kr]5s^24d^105p^5

Give the ground state electron configuration for Pb.

[Xe] 6s^2 4f^14 5d^10 6p^2

Predict the charge that an ion formed from sulfur would have

2- Look at #52^^^

How many valence electrons do the alkali metals possess?

1 VE

List all orbitals from 1s through 5s according to increasing energy for multielectron atoms.

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

Rubidium belongs to the ________ group of the periodic table.(Rb)

Alkali Metal

Place the following in order of increasing IE1. (Ionization Energy) > > > ^ ^ ^ N F As

As < N < F

Which of the following elements is NOT a metal?

Ba Xe **** Mg Ga Pb

A certain element forms an ion with 54 electrons and a charge of +2. Identify the element.

Ba--> Atomic #(+2) Group 2 which loses two electrons... +=- and -=+

Which of the following elements is a nonmetal?

C

Which element is a transition metal?

Ca Xe Cr****** Pb

Place the following elements in order of increasing atomic radius. P Ba Cl

Cl<P<Ba

Choose the statement that is TRUE.

Core electrons effectively shield outer electrons from nuclear charge.

Which statement is true about effective nuclear charge?

Effective nuclear charge increases as you move to the right across a row in the periodic table.

main group metal tends to lose electrons, forming a cation with the same number of electrons as the nearest noble gas in the periodic table. A main group nonmetal tends to gain electrons, forming an anion with the same number of electrons as the nearest noble gas. The various groups gain or lose electrons as summarized in the following table:

Group Tendency Charge 1 (1A) Lose one electron +1CHarge 2 (2A) Lose two electrons +2Charge 13 (3A) Lose three electrons +3CHarge 15 (5A) Gain three electrons -3Charge 16 (6A) Gain two electrons -2Charge 17 (7A) Gain one electron -1Charge 18 (8A) Rarely gain or lose electrons 0 Charge

How many valence electrons do the alkaline earth metals possess?

Group 2: 2 VE

Place the following in order of decreasing metallic character. P As K

K > As > P.... the most metallic are of the periodic table is the bottom left corner.. arrows go down and to the left <(down) , <----

Name an element in the fourth period (row) of the periodic table with a complete outer shell.

Kr

Which reaction below represents the electron affinity of Li?

Li(g) + e- → Li-(g)

Choose the element with the more negative (more exothermic) electron affinity from each of the following pairs. Na or Rb B or S C or N Li or F

Na S C F

Place the following in order of increasing metallic character. Rb Cs K Na

Na < K < Rb < Cs

Which reaction below represents the first ionization of O?

O(g) → O+(g) + e- Na --> Na+ + e-

Which of the following elements is a good conductor of heat and electricity?

copper****** argon bromin carbon

What are the observed periodic trends in electron affinity?

for main-group elements, electron affinity generally becomes more negative as you move to the right across a row there is not a corresponding trend in electron affinity going down a column

What is the general trend in first ionization energy as we move down a column in the periodic table? As we move across a row?

ionization energy decreases Ionization energy generally increases as you move to the right across a period.

The element that corresponds to the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5 is ________.

iron titanium chromium ***** manganese vanadium

Which of the following does not describe a nonmetal?

tend to gain electrons relatively unreactive ********** poor conductor of electricity found in the upper right hand corner of the periodic table poor conductor of heat

How many protons does the As3- ion possess?

33

Identify a violation of the Pauli exclusion principle opened hint In an orbital diagram, the arrows are used to indicate the relative spin of an electron (indicative of its value). Which of the following correctly describes a violation of the Pauli exclusion principle?

Arrows in the same orbital with the same direction.The Pauli exclusion principle is violated only when two electrons in the same orbital have like spins. This means that they have the same set of quantum numbers.

No two electrons can have the same four quantum numbers is known as the

Aufbau principle Heisenberg uncertainty principle Pauli exclusion principle ********* Hund's rule

Iodine belongs to the ________ group of the periodic table.

Halogen

The shielding of electrons gives rise to an effective nuclear charge, Zeff , which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?

How many protons and how many inner (nonvalence) electrons does a neutral boron atom have? 5,2 How many protons and how many inner (nonvalence) electrons does a neutral oxygen atom have? 8,2 +3 and +6

Who is credited with arranging the periodic table?

Robert Boyle Dmitri Mendeleev***** Johannes Nicolaus Brønsted Amedeo Avogadro Thomas Martin Lowry

For which of the following elements will gaining an electron be the most exothermic process? Electron affinities in general become more negative moving from left to right across a row of the periodic table.

S*** Si Al Mg

Which of the following elements is a metalloid?

Silicon

Choose the more metallic element from each of the following pairs.

Sr or Sb--> Sr As or Bi--> Bi Cl or Se--> Se S or As--> As

Which reaction below represents the second ionization of Sr?

Sr+(g) → Sr2+(g) + e- Na+ --> Na2+ + e-

Which of the following elements has chemical properties similar to polonium?

Sulfur.. Both in group 16.. vertical groups have similar chemical properties

Identify the element that has a ground state electronic configuration of [Kr]5s2 4d5.

Tc ** Ru Mn Nb

Which of the following sets contains elements that will form ions with a charge of 2−?

Te, S, and O...... The main-group elements tend to form ions that have the same electron configuration as the nearest noble gas. Recall that electrons can be either lost or gained.

Any other order of filling the electrons represents a violation of the aufbau principle.

The order in which electrons would fill in the subshells is 1s→2s→2p→3s→3p→4s→3d→4p→5s→4d and so on. The electrons will first fill the 1s lower energy subshell completely and then the 2s higher energy subshell will be filled completely followed by subshells 2p, 3s, and so on in order of their increasing energies.

restrictions on the principal quantum number

The principal quantum number n is restricted to integers greater than zero.

the restrictions on the spin quantum number

The spin quantum number is listed last in a set of four quantum numbers. One way to quickly identify invalid sets is to find ones in which the last value is not 1/2 or −1/2.

Which of the following is the term used to describe a set of elements whose properties tend to be largely predictable based on their position on the periodic table?

Transition Main-group ***** Inner transition Period

Barium belongs to the ________ group of the periodic table. (Ba)

an atom that has gained an electron

Identify an anion.

an atom that has gained an electron

restrictions on the magnetic quantum number

ℓ=0 m = 0 ℓ=1 m = -1, 0, or 1 ℓ=2 m = −2,−1, 0, 1, or 2

The ________ is a change in energy associated with gaining an electron in the gaseous state for an atom or ion.

electron affinity

Mendeleev's table is based on the periodic law, which states that when elements are arranged in order of increasing ______, their properties recur periodically. Mendeleev arranged the elements in a table in which_______increased from left to right and elements with similar properties fell in the same ________.

mass;mass;columns

Semiconductors are

metalloids

Which set of four quantum numbers corresponds to an electron in a 4p orbital?

n=4,l=1, ml=0, ms=1/2 The 4 in 4p indicates that n=4 . Since this is a p orbital, l is 1. The possible values of mlfor l=1are −1, 0, and 1, so ml=0 is allowed. Lastly, ms can be either 1 2 or − 1 2 .

According to Hund's rule, the electrons will arrange in the degenerate set of orbitals with one electron in each orbital with like spins before any pairing occurs. So for Hund's violation to occur the subshell must have a degenerate set of orbitals. In which type of subshell could a Hund's rule violation occur?

p and d; since s subshells have only one orbital, it is not possible to violate Hund's rule, which pertains to sets of degenerate orbitals. In all other subshells, the electrons are added to each orbital in the degenerate set one at a time with like spins before any pairing occurs. For Hund's rule to apply, there must be a set of degenerate orbitals. Recall that for the s subshell there is only one possible value for mℓ and therefore the s subshell contains only one orbital.

Which of the following does NOT describe a metal?

tends to gain electrons******* forms ionic compounds with nonmetals found on the left side of the periodic table. good conductor of heat good conductor of electricity

Explain the relationship between a main-group element's lettered group number (the number of the element's column) and its valence electrons.

the lettered group number of a main-group element is equal to the number of valence electrons for that element.

restrictions on the angular momentum quantum number

ℓ has integer values from 0 to n−1. In other words, ℓ must be an integer that is less than n, but it cannot be negative.