Chemistry chapter 6 and 7

In their compounds, the charges on the alkali metals and the alkaline earth metals are ________ and ________, respectively.

+1, +2

For orbitals of identical energy, electrons enter empty orbitals whenever possible is ________

- Hund's rule

hich of the following is not a valid set of four quantum numbers? (n, l, ml, ms) 1, 0, 0, +1/2 2, 1, 0, -1/2 2, 0, 0, +1/2 1, 1, 0, +1/2 3, 1, -1, -1/2

1, 1, 0, +1/2

An electron cannot have the quantum numbers n = ________, l = ________, ml = ________. 3, 1, -1 2, 1, -1 3, 2, 1 2, 0, 0 1, 1, 1

1, 1, 1

Each d-subshell can accommodate a maximum of ________ electrons. 3 10 6 2 5

10

The 4d subshell in the ground state of atomic xenon contains ________ electrons. 10 6 2 8 36

10

For how many electrons in an Ne atom does = 1 and = 1? 0 10 2 6 1

2

The 3p subshell in the ground state of atomic silicon contains ________ electrons. 2 10 36 8 6

2

hich is not an acceptable value for the principle quantum number if n = 2.0? -2 2.0 -1 0 1

2.0

Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? 2d None of these 2s 2p All of these

2d

The principal quantum number of the first d subshell is ________. 4 0 3 1 2

3

Which one of the following is not a valid value for the magnetic quantum number of an electron in a 5d subshell? 1 0 3 -1 2

3

hat is the lowest numbered principal shell in which d orbitals are found? 2 5 1 4 3

3

ow many orbitals are there in the 4p subshell? 1 3 2 5 4

3

Which one of the following is an incorrect orbital notation? 4dxy 4s 2s 3f 3py

3f

How many subshells are there in an energy level with n = 4? 2 5 4 1 3

4

The ________ subshell contains only one orbital. 6f 4s 3d 5d 1p

4s

he ________ subshell contains only one orbital. 6f 4s 5d 1p 3d

4s

How many d orbitals reside in d subshell? 1 3 7 2 5

5

The electron configuration of the valence electrons of an atom in its ground state is ns2np3. This atom is a group ________ element.

5A

how many orbitals are there of the 4f type? 7 9 2 3 5

7

Elements in group ________ have an np5 electron configuration in the outer shell.

7A

at is the total number of orbitals is the principal shell n = 3? 4 8 18 1 9

9

here are ________ orbitals in the third shell. 25 4 1 16 9

9

Which of the following is an f-block element? A) Ce B) Be C) N D) Au E) Co

A) Ce

Which of the following is a d-block element? A) Cu B) Cs C) Be D) O E) No

A) Cu

Which of the following is an s-block element? A) K B) Fe C) O D) Sm E) Mo

A) K

_____ are soft, metallic solids.

Alkali metals

Of the choices below, which gives the order for first ionization energies? S > Si > Cl > Al > Ar Ar > Cl > S > Si > Al Cl > S > Al > Ar > Si Al > Si > S > Cl > Ar Cl > S > Al > Si > Ar

Ar > Cl > S > Si > Al

Which element has the greatest (most negative) electron affinity? A) C B) O C) Si D) S

B) O

Which of the following set is an acceptable set of quantum numbers? A) n = 1, l = 0, ml = 0 B) n = 3, l = 1, ml = -1 C) n = 0, l = 0, ml = 0 D) n = 2, l = 1, ml = 2

B) n = 3, l = 1, ml = -1

hich ion below has the largest radius? Na+ Br- F- K+ Cl-

Br-

What is the lowest-numbered principal shell in which ml = 1 is possible? A) 0 B) 1 C) 2 D) 3

C) 2

How many electrons are there in a half-filled d subshell? A) 1 B) 3 C) 5 D) 7 E) 4

C) 5

How many electrons are there in a filled p subshell? A) 2 B) 3 C) 6 D) 8 E) 18

C) 6

Which set of elements is not in order of increasing atomic radius (smallest one first, etc.)? A) Na, K, Rb B) F, S, As C) C, N, O D) Br, Se, As

C) C, N, O

All of the following are ionic compounds except ________. Be(OH)2 NiCl2 Sr3N2 CH4 K2O

CH4

Which one of the following compounds would produce an acidic solution when dissolved in water? CO2 MgO SrO CaO Na2O

CO2

Of the following atoms, which has the largest first ionization energy? Rb K Ca Ba Sr

Ca

Which equation correctly represents the electron affinity of calcium? Ca- (g) Ca (g) + e- Ca (g) + e- Ca- (g) Ca+ (g) + e- Ca (g) Ca (g) Ca- (g) + e- Ca (g) Ca+ (g) + e-

Ca (g) + e- Ca- (g)

Of the following elements, ________ has the most negative electron affinity. Br I S Se Cl

Cl

_______ is isoelectronic with argon. F- P4- K- Ca Cl-

Cl-

How many electrons are there in a filled n = 3 principal shell? A) 2 B) 6 C) 8 D) 18 E) 32

D) 18

How many subshells are there in an energy level with n = 4? A) 1 B) 2 C) 3 D) 4

D) 4

According to the subshell filling order which sublevel is filled after the 5s sublevel? A) 5p B) 4f C) 3d D) 4d E) 5d

D) 4d

Which of the following sets of elements is arranged in the correct order of decreasing ionization energy (highest energy first, etc.)? A) Rb, K, Ca B) As, S, F C) K, Na, Li D) Cl, Br, I

D) Cl, Br, I

_____ is the energy change that occurs when an electron is added to a gaseous atom:

Electron affinity (EA)

________ describes the distribution of electrons among the various orbitals in the atom.

Electron configuration

Of the following elements, ________ has the most negative electron affinity. F I Cl Br H

F

_______ is isoelectronic with helium. N3- H+ B3- H H-

H-

________ is a unique element and does not truly belong to any family. Nitrogen Helium Hydrogen Radium Uranium

Hydrogen

List seven nonmetals that exist as diatomic molecules in their elemental forms.

Hydrogen Nitrogen Oxygen Fluorine Chlorine Iodine Bromine

All of the subshells in a given shell have the same energy in the hydrogen atom. In a many-electron atom, the subshells in a given shell do not have the same energy. Why?

Hydrogen only has one electron. Other atoms with many electrons fill up different shells that are on different energy levels.

Which one of the following atoms has the largest radius? Te In Sb I Sn

In

______: the energy required to remove an electron from a ground-state gaseous atom.

Ionization energy

_____: species that have the same number of electrons

Isoelectronic

Which element would be expected to have chemical and physical properties closest to those of rubidium? Fe Cu Ca S K

K

Which one of the following is a metal? Si S Li He I

Li

Which metal is a liquid at room temperature?

Mercury (Hg)

f the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? Mg > Na > P > Si > Ar Na > Mg > Si > P > Ar Ar > P > Si > Mg > Na Ar > Si > P > Na > Mg Si > P > Ar > Na > Mg

Na > Mg > Si > P > Ar

hich of the following correctly lists the five atoms in order of increasing size (smallest to largest)? Ne < Si < O < S < Ge Ne < Ge < Si < S < O Ge < Si < S < O < Ne Ne < O < S < Si < Ge Ne < S < O < Si < Ge

Ne < O < S < Si < Ge

In which set of elements would all members be expected to have very similar chemical properties? Ne, Na, Mg N, O, F O, S, Se Na, Mg, K S, Se, Si

O, S, Se

_______ - no two electrons in the same atom may have the same four quantum numbers, in other word, Orbitals hold a maximum of two electrons, and spins must be opposed

Pauli exclusion principle

the element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ________. B Ge Sn As Si

Si

Which one of the following is not true about the alkali metals? They have the lowest first ionization energies of the elements. They are low density solids at room temperature. They all readily form ions with a +1 charge. They are very reactive elements. They all have 2 electrons in their valence shells.

They all have 2 electrons in their valence shells.

A group of ions all containing the same number of electrons constitutes an isoelectronic series. True False

True

Electron affinity measures how easily an atom gains an electron. True False

True

When the value of n is greater than or equal to 3, electrons can reside in d orbitals. True False

True

orbital is best defined as a region in space in which there is a high probability of finding an electron. a circular path that an electron takes around a nucleus. an orientation of the nucleus and electron in an atom. an energy level for electrons. a node where the probability of finding an electron is small.

a region in space in which there is a high probability of finding an electron.

Which of the following is not a characteristic of metals? ductility low ionization energies malleability acidic oxides These are all characteristics of metals.

acidic oxides

l of the ________ have a valence shell electron configuration ns^1. alkaline earth metals noble gases halogens alkali metals chalcogens

alkali metals

The ________ quantum number defines the shape of an orbital. magnetic spin principal psi angular momentum

angular momentum

A wave function with a given set of these three quantum numbers is called an_________

atomic orbital

[Xe]6s2 is the electron configuration for ________.

barium

Of the elements below, ________ is the most metallic. barium cesium sodium magnesium calcium

cesium

Sodium is much more apt to exist as a cation than is chlorine. This is because ________. chlorine has a greater electron affinity than sodium does chlorine is a gas and sodium is a solid chlorine has a greater ionization energy than sodium does chlorine is more metallic than sodium chlorine is bigger than sodium

chlorine has a greater ionization energy than sodium does

Atomic radius generally increases as we move ________. down a group and from left to right across a period up a group and from right to left across a period up a group and from left to right across a period down a group and from right to left across a period down a group; the period position has no effect

down a group and from right to left across a period

A negative electron affinity means that the process is ______

exothermic

he angular momentum quantum number is 3 in ________ orbitals. f d s a p

f

Alkaline earth metals ________. exist as triatomic molecules form monoanions form halides with the formula MX form basic oxides have the smallest atomic radius in a given period

form basic oxides

All of the halogens ________. tend to form positive ions of several different charges exhibit metallic character form salts with alkali metals with the formula MX tend to form negative ions of several different charges exist under ambient conditions as diatomic gases

form salts with alkali metals with the formula MX

Which noble gas has the highest first ionization energy?

helium

Atomic radii _____ from top to bottom and ______ from left to right

increase, decrease

As successive electrons are removed from an element, the ionization energy ________.

increases

What are the elements called that are located between the metals and nonmetals?

metalloids

In nature, the noble gases exist as ________. monatomic gaseous atoms alkali metal salts solids in rocks and in minerals the gaseous fluorides the sulfides

monatomic gaseous atoms

Which quantum number determines the energy of an electron in a hydrogen atom? n l n and l ml E

n

Which of the following sets is not an acceptable set of quantum numbers. n = 7, = 3, = +3 n = 1, = 0, = 0 n = 3, = 1, = -3 n = 2, = 1, = -1 n = 2, = 1, = +1

n = 3, = 1, = -3

The total number of orbitals in a shell is given by ________. 2l + 1 2n 2n + 1 I^2 n^2

n^2

The______ uses boxes to represent orbitals within subshells and arrows to represent electrons.

orbital diagram

All of the group VIA elements are solids except ________.

oxygen

All of the orbitals in a given electron shell have the same value as the ________ quantum number. magnetic angular momentum principal spin psi

principal

All of the orbitals in a given subshell have the same value as the ________ quantum number. angular momentum and magnetic principal angular momentum magnetic principal and angular momentum

principal and angular momentum

If orbitals having the same value of n, then these orbitals are in the same _____

principle shell

The wave functions for the hydrogen atom contain three parameters that must have specific integral values called _____

quantum numbers

If orbitals having the same value of n and the same value of l, then these orbitals are in the _____

same subshell.

Nonmetals can be ________ at room temperature. solid or liquid liquid or gas liquid only solid only solid, liquid, or gas

solid, liquid, or gas

Element M reacts with oxygen to form an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M could be ________. nitrogen bromine selenium germanium strontium

strontium

The atomic radius of main-group elements generally increases down a group because ________. both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases effective nuclear charge decreases down a group the principal quantum number of the valence orbitals increases effective nuclear charge increases down a group effective nuclear charge zigzags down a group

the principal quantum number of the valence orbitals increases