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Flashcards in Chapter 8 Test Deck (25)
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1
Q

The Stern-Gerlach experiment, showing two different electron spins, was first carried out using silver atoms ( [Kr] 4d105s1 ). The experiment will work with other elements, but only certain ones. Which of the following elements would demonstrate the effect seen in the Stern-Gerlach experiment?

A

potassium

2
Q

The graph shows the result of an photoelectron spectroscopy experiment for neon. The graph plots numbers of electrons ejected against their excess kinetic energy. Which part of this graph would give us information about the ionization energy for this element assuming you know the energy of the photon used?

A

The location of the right-hand peak.

3
Q

How does the size of the cation compare to its corresponding atom?

A

The cation is smaller.

4
Q

Within a period, what happens to the size of an atom as the atomic mass increases?

A

The atom gets smaller.

5
Q

Why is it difficult to measure the size of an atom?

A

The outer edge of an atom is difficult to determine.

6
Q

Indium (a metal that in its pure form emits a high-pitched “scream” when bent) comes immediately after cadmium ( [Kr] 4d105s2 ) on the periodic table. What is the electron configuration for indium

A

[Kr] 4d10 5s2 5p1

7
Q

An ion has the electron configuration 1s22s22p6 and a double negative charge. What element is it?

A

O

8
Q

What forces need to be considered in determining where an electron might be in an atom?

A

The potential energy, the kinetic energy and the repulsion of like-charged particles

9
Q

What is an effective nuclear charge?

A

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

10
Q

Which of the following would have the most negative energy?

A

An electron that is in a 2s orbital

11
Q

There are no known compounds of neon, a noble gas. Which of the following is the best explanation of the inert nature of neon?

A

It is both harder to add an electron to and remove an electron from neon, thus no compounds readily form.

12
Q

Which of the following best illustrates the aufbau principle?

A

Electrons filling up existing orbitals in an expected arrangement

13
Q

Which of the following characteristics is most alike in elements that have similar chemical properties?

A

Valence electron configuration

14
Q

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

A

+2

15
Q

Which of the following best defines isoelectronic?

A

having the same number of electrons

16
Q

Which of the follow explains why there is a difference in first ionization energy between nitrogen and oxygen?

A

Nitrogen has a more stable electron configuration

17
Q

Which of the following is used to describe the ionization energy for hydrogen?

A

Schrödinger equation

18
Q

How does the size of an atom when it accepts an electron compare to the size of its ion?

A

The ion is larger in size than its parent neutral atom.

19
Q

What is electron affinity?

A

The energy change that occurs when an atom gains an electron.

20
Q

How do electrons react to other electrons?

A

They are repelled by each other.

21
Q

Which of the following periodic trends cannot be directly measured?

A

Electronegativity

22
Q

Electronegativity describes the ability of an atom to attract additional electron density to itself. Electronegativity would not help predict:

A

Solubility of a substance in water.

23
Q

Which of the following pairs of metals and nonmetals would combine in a 1:1 ratio in a chemical reaction?

A

Rubidium and Iodine

24
Q

Using what you know about the periodic table and the properties of elements, determine which of the following compounds will not exist.

A

NaCl2

25
Q

Metals are generally involved in the formation of which of the following?

A

Cations

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