General Education

How many elements cannot have a noble gas configuration

How many elements cannot have a noble gas configuration?

Question 1 options:

0

1

2

3

Question 2 (1 point)

Which of these describes sheilding?

Question 2 options:

core electrons shield valence electrons from the positive charge of the nucleus so that the valence electrons experience a charge less than the total nuclear charge.

core electrons shield valence electrons from the nucleus, but the valence electrons experience the total nuclear charge.

valence electrons shield core electrons from the positive charge of the nucleus so that the core electrons experience a charge less than the total nuclear charge.

valence electrons shield core electrons from the nucleus, but the valence electrons experience the total nuclear charge.

Question 3 (1 point)

The properties of an element are determined by (choose the best answer).

Question 3 options:

number of neutrons

number of protons

number of electrons

its valence electron configuration

number of valence electrons

Question 4 (1 point)

For increasing metallic character, make two arrows pointing toward _________on the periodic table

Question 4 options:

Fr

F

Question 5 (1 point)

When determining the electron configuration for an ion, which of these electrons should always be removed first?

Question 5 options:

the last electrons you listed

the highest energy electrons

electrons in the outermost (valence) shell -with the highest n value

Question 6 (1 point)

Which of these has the highest first ionization energy?

Question 6 options:

B

N

O

F

C

He

Question 7 (1 point)

When writing the noble gas configuration for Gd (#64) which noble gas do you use?

Question 7 options:

Og

Xe

Kr

He

Ne

Rn

Ar

Question 8 (1 point)

When writing the noble gas configuration for Aluminum, which noble gas do you use?

Question 8 options:

He

Ar

Xe

Kr

Rn

Ne

Og

Question 9 (1 point)

According to Coulomb's law, the attraction between a proton and an electron in an atom ____________with increasing_____________

Question 9 options:

decreases; their sizes

increases; distance between their centers

decreases; their charges

decreases; distance between their centers

decreases; their sizes

Question 10 (1 point)

Each element has multiple ionization energies. The first ionization energy is the energy required to pull off one electron. The second ionization energy is the energy required to remove one more electron after that, and so on. If you look at a list of ionization energies, for any element, you find a big jump______________________

Question 10 options:

between the first and second ionization

the ionization energy after the resulting ion has a noble gas configuration because a noble gas configuration is already stable

between the second and third ionization 

Question 11 (1 point)

What is the electron configuration for bromide ion?

Question 11 options:

[Ar]4s23d104p6

[Ar]4s23d104p7

[Kr]

[Ar]

Question 12 (1 point)

Which of these decreases in magnitude as you go across a period on the periodic table?

Question 12 options:

Zeff

ionization energy

electron affinity

atomic radius

electronegativity

Question 13 (1 point)

Which of these statement describes one of the exceptions to the ionization energy trend? 

Question 13 options:

column 2A has a lower ionization energy than column 3A because s electrons are farther from the nucleus, and therefore harder to remove than p electrons.

column 2A has a lower ionization energy than column 3A because s electrons are closer to the nucleus, and therefore harder to remove than p electrons.

column 2A has a higher ionization energy than column 3A because s electrons are farther from the nucleus, and therefore harder to remove  than p electrons.

column 2A has a higher ionization energy than column 3A because s electrons are closer to the nucleus, and therefore harder to remove than p electrons.

Question 14 (1 point)

The driving force for elements form ions (whether positive or negative) is 

Question 14 options:

to obtain a noble gas configuration

to become charged instead of neutral

To release energy

Question 15 (1 point)

Valence electrons are always all except

Question 15 options:

electrons in the outermost shell

electrons of the highest energy

s electrons in the shell with the highest number n

p electrons in the shell with the highest number n

Question 16 (1 point)

Which of these is not isoelectronic with the others?

Question 16 options:

Cl-

Na+

S2-

Ar

Br-

Mg2+

Question 17 (1 point)

Calculate Zeff for a lithium ion. You may want to draw one so that you can identify the core electrons and the valence electrons.

Question 17 options:

+3

+2

0

-1

+4

+1

Question 18 (1 point)

Which of these describes penetration?

Question 18 options:

The wavefunction of an electron from a higher energy orbital overlaps the wavefunction of a lower energy orbital.

The wavefunction of an electron from a lower energy orbital overlaps the wavefunction of a higher energy orbital.

Electrons attract each other such that valence electrons are closer to the nucleus.

Electrons repel each other such that valence electrons are farther from the nucleus.

Question 19 (3 points)

Arrange these from biggest to smallest

Question 19 options:123noble gas123cation123anion

Question 20 (1 point)

Which of these statements describes one of the exceptions to the ionization energy trend? 

Question 20 options:

group 5A has a lower ionization energy than group 6A because group 5A has a half-filled p subshell, which is aless stable confirmation than group 6A, in  which the p subshell is neither half full nor completely full.

group 5A has a higher ionization energy than group 6A because group 5A has a half-filled p subshell, which is aless stable confirmation than group 6A, in which which the p subshell is neither half full nor completely full.

group 5A has a higher ionization energy than group 6A because group 5A has a half-filled p subshell, which is a more stable confirmation than group 6A, in which the p subshell is neither half full nor completely full.

group 5A has a lower ionization energy than group 6A because group 5A has a half-filled p subshell, which is a more stable confirmation than group 6A, in which the p subshell is neither half full nor completely full.

Question 21 (1 point)

The ionization energy__________________

Question 21 options:

is the energy it takes to remove an electron from an atom and is a positive number

is the energy it takes to add an electron to an atom and is a negative number.

is the energy it takes to add an electron to an atom and is a positive number.

is the energy it takes to remove an electron from an atom and is a negative number.

Question 22 (1 point)

Which element has the electron configuration

1s22s22p63s23p64s23d103p65s24d105p66s24f145d106p67s25f146d7

Question 22 options:

Ds #110

Ra #88

Tr #77

Hs #108

Mt #109

Question 23 (1 point)

What is the electron configuration of carbon?

Question 23 options:

1s22s12p3

1s22s4

1s22s22p2

1s22p4

Question 24 (1 point)

When writing the noble gas configuration for Ts (#117), which noble gas do you use?

Question 24 options:

Og

Xe

Ne

Kr

Rn

He

Ar

Question 25 (3 points)

Match the families to the blocks on the periodic table.

Question 25 options:1234

inner transition metals

1234

lanthanides

1234

alkaline earth metals

1234

alkali metals

1234

nonmetals

1234

halogens

1234

transition metals

1234

semimetals

1234

noble gases

1234

actinides

1.

s-block

2.

p-block

3.

d-block

4.

f-block

Question 26 (1 point)

The noble gas configuration for Aluminum ion is ?

Question 26 options:

Kr

Ar

Ne

Og

Rn

He

Xe

Question 27 (1 point)

When writing electron box diagrams, which of these is false?

Question 27 options:

Electrons in the same subshell can have parallel spins

Electrons in the same orbital can have parallel spins

Question 28 (1 point)

The electron affinity__________________

Question 28 options:

is the energy it takes to remove an electron from an atom and is a positive number

is the energy it takes to add an electron to an atom and is a positive number.

is the energy it takes to add an electron to an atom and is a negative number.

is the energy it takes to remove an electron from an atom and is a negative number.

Question 29 (1 point)

Atomic radii are determined by

Question 29 options:

the number of valence electrons; they repel each other and increase the ionic radius.

the electronegativity; more electronegative atoms attract more electrons and therefore are greater in size.

Zeff: the higher nuclear charge pulls the electrons closer to the nucleus to decrease the size of the atom.

Question 30 (1 point)

Which of these is not isoelectronic with the others?

Question 30 options:

Na+

S2-

Mg2+

Ar

Cr2+

Question 31 (1 point)

What is the electron configuration for Calcium ION?

Question 31 options:

[Ar]4s1

[Ar]

[Ar]4s23d2

[Ar]4s2

Question 32 (1 point)

What is the electron configuration for Fe2+ ion?

Question 32 options:

 [Ar]4s23d4

[Ar] 3d6

[Ar]

[Ar]3d10

[Ar]4s23d6

Question 33 (1 point)

Electronegativity is 

Question 33 options:

the ability to donate electrons to another atom

the ability to donate protons to another atom

the ability to attract protons to oneself

the ability to attract electrons to oneself

Question 34 (1 point)

Which of these is diamagnetic?

Question 34 options:

Se

Si

Cl

Ar

Question 35 (1 point)

Which element has an electron configuration of 1s22s22p63s23p64s23d103p65s24d4 

Question 35 options:

W

Mo

Ba

Cr

Sr

Question 36 (1 point)

Which of these have ions with noble-gas configurations?

Question 36 options:

actinides

main group elements

lanthanides

transition metals

Question 37 (1 point)

Zeff increases accross a period (for the main group elements) because

Question 37 options:

the nuclear charge decreases with the number of protons in the atoms, but the number of shielding electrons inreases.

the nuclear charge increases with the number of protons in the atoms, but the number of shielding electrons inreases.

the nuclear charge decreases with the atomic number, but the number of shielding electrons stays the same.

the nuclear charge increases with the atomic number, but the number of shielding electrons stays the same.

Question 38 (1 point)

Which is true about Zeff

Question 38 options:

it is the nuclear charge minus the total charge of the rest of the electrons in the atom  

it is the nuclear charge minus the total charge of the rest of the electrons that penetrate the nucleus of the atom

it is the nuclear charge minus the total charge of the electrons in lower energy shells 

it is the nuclear charge minus the total charge of the electrons in higher energy shells

Question 39 (1 point)

Using the trend for EA (not the exceptions), select the element that has the highest electron affinity)

Question 39 options:

F

N

O

Ar

Question 40 (1 point)

Which of these decreases in magnitude as you go right on the periodic table?

Question 40 options:

atomic radius

electronegativity

electron affinity

ionization energy

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