Chapter 8 Practice Test Flashcards Preview

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Flashcards in Chapter 8 Practice Test Deck (25)
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1
Q

What are legitimate values for the spin quantum number, ms?

A

−½ and +½

2
Q

Which of the following best states the Pauli exclusion principle?

A

Each electron in an atom must have a unique set of quantum numbers describing it.

3
Q

Which statement about Stern and Gerlach’s experiments with silver atoms is not correct?

A

The experiments showed that the first three quantum numbers were the same for every electron in a given silver atom.

4
Q

What is an effective nuclear charge?

A

The charge experienced by electrons in outer energy levels through electron shielding

5
Q

Which of the following is the best description of electron shielding?

A

Electron shielding is the decrease in the effective nuclear charge experienced by an electron in an outer energy level, due to the interaction of electrons at lower levels with the nucleus.

6
Q

How many electrons can fit in any given orbital?

A

2

7
Q

Which of the following is the best explanation of why it is harder to remove an electron from an atom of neon than an atom of fluorine?

A

It is harder to remove an electron from neon than fluorine because of increased nuclear charge (Z = 10).

8
Q

Which of the following represents the electron configuration for carbon?

A

This is the correct number of electrons and in the correct orientation. This diagram shows that the electrons in the 2p orbital are entering separate orbitals and have parallel spins.

9
Q

What is the ground state electron configuration for oxygen?

A

1s22s22p4

10
Q

What is the maximum number of electrons in a 3d set of orbitals?

A

10

11
Q

What is the electron configuration of sodium ion (Na+ )?

A

[ Ne]

12
Q

What is the most common oxidation state for alkaline earth metals?

A

+2

13
Q

Elements with partially-filled 4f orbitals are part of which of the following?

A

The lanthanide series

14
Q

Which of the following is the periodic trend for size of an atom?

A

As you move down a group, the size of the atoms increases because each atom has a larger nucleus and more electrons. As you move across the periodic table from left to right, the nuclear charge increases causing the electrons to move in closer to the nucleus, which causes the size of the atom to decrease.

15
Q

What is the maximum number of electrons that may be found in a 3p energy sublevel?

A

6

16
Q

In which of the following lists are the elements arranged in order of increasing ionization energies?

A

Fe, Co, Ni, Cu

17
Q

What is the total number of electrons that can be held in the 2p orbitals?

A

6

18
Q

Why does electron affinity generally increase as you go from left to right across the periodic table?

A

The elements on the right side of periodic table usually have a larger number of protons and a smaller atomic radius than elements on the left side of the periodic table.

19
Q

Which of the following groups of elements is most likely to have a valence of 2–?

A

Chalcogens (the oxygen group)

20
Q

Which of the following is the least electronegative element and the most electronegative element, respectively?

A

francium, fluorine

21
Q

What elements have relatively small electronegativity values?

A

Electropositive elements

22
Q

Which element would be expected to have the highest first ionization energy?

A

F

23
Q

Which of the following properties is shared by the alkali metals and the alkaline earth metals?

A

They are not found in their elemental state in nature.

24
Q

In a compound, what is the oxidation number of magnesium?

A

2+

25
Q

In most of the transition metals, the d orbitals fill up after the s orbitals of the next higher principal quantum number. Why does this occur?

A

Because the s orbitals have a lower energy

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