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Flashcards in Chapter 6 Test Deck (32)
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1
Q

What is ionization energy?

A

The amount of energy required to remove an electron from an atom or ion. (This forms a positive ion.)

2
Q

State the trends for electron affinity. Don’t forget the exceptions! b. Explain why it has these trends.

A

a. Electron affinity increases (becomes more negative) across a period and decreases down a group. The exception is the noble gases, which have little or no electron affinity. B. Electron affinity increases across a period because protons are being added to the nucleus. This makes the nucleus more positive, which gives it a greater attraction for electrons. This means that it’s easier for an atom to gain a new electron. It decreases down a group because electron shielding blocks the nucleus, so it can’t attract new electrons as easily. Also, the electrons are farther from the nucleus, where the pull from the nucleus isn’t as strong.

3
Q

Explain what “Coulomb’s law” is.

A

The closer opposite charges are to one another, the stronger the attraction between them is. The farther apart opposite charges are, the weaker the attraction.

4
Q
  1. List one property of the actinides. Where are the actinides?
A

Nuclear structures are more important than electron configurations, all are radioactive. Located in first row of f-block, or element #90-103.

5
Q

List two properties of metalloids.

A

Semiconductors, conduct better than nonmetals but not as well as metals, solid at room temp.

6
Q
  1. What is electron affinity?
A

The energy emitted upon the addition of an electron to an atom or group of atoms in the gas phase. (More neg. e- affin. Means more energy is given off, which means the atom has a stronger attraction for new electrons.)

7
Q

State the trends for ionization energy. b. Explain why it has these trends.

A

Ionization energy increases across a period and decreases down a group. B. Ionization energy increases across a period because protons are being added to the nucleus. This makes the nucleus more positive, which gives it a greater attraction for electrons. This means that it’s harder (takes more energy) to remove an electron. It decreases down a group because electron shielding blocks the nucleus, so it doesn’t hold onto electrons as strongly. Also, the electrons are farther from the nucleus, so they are easier to remove (it takes less energy to remove them).

8
Q

State two properties of noble gases.

A

all gases, very low reactivity, full outer energy level

9
Q
  1. Why don’t noble gases fit the trend?
A

The already have a full outer energy level (stable octet of electrons) so they don’t want to add any new electrons. If you were to add a new electron to a noble gas, you would have to start an entire new energy level.the noble gases have the lowest (most positive) electron affinity. (Remember, electron affinity is negative.)

10
Q
  1. What does it mean to say that something is periodic?
A

It has a repeating pattern.

11
Q

Explain why ionization energy and electron affinity decrease as you move from top to bottom. Explain in terms of the nucleus’s attraction for electrons. Be sure to discuss electron shielding and Coulomb’s law.

A

As you move down the column, the nucleus has a weaker attraction for outer electrons. This is because (1) e- shielding increases because you have more core electrons blocking the pull of the nucleus, and (2) e- are farther from the nucleus, making the attraction weaker, which is Coulomb’s law. A weaker attraction for outer electrons means that (1) outer e- are easier to remove (low IE) and there is not much attraction for new electrons (low e- affin.).

12
Q

Explain why nuclear charge increases as you move from left to right across the periodic table.

A

As you move from left to right, more protons are added to the nucleus. That means the nucleus has more positive charge.

13
Q
  1. Explain why ionization energy and electron affinity increase as you move from left to right. Explain in terms of the nucleus’s attraction for electrons.
A

As you move from left to right, you add protons to the nucleus. That makes the positive nuclear charge stronger, which pulls on the electrons more tightly. This makes it harder to remove electrons (high IE) and easier to pull in new electrons (high e- affinity).

14
Q

Why do elements in the same group have similar properties?

A

They have the same outer energy level electron configuration.

15
Q

List four properties of alkali metals.

A

React vigorously with water to produce alkaline solutions and hydrogen gas, metallic properties, very reactive, soft, shiny but dull quickly when cut, only one electron in outer E level, lose the e- to become like a noble gas, become plasmas in the gaseous state at high temps

16
Q

Name two properties of alkali metals.

A

react with water to make alkaline (basic) solutions, one electron in their outer energy level, soft (can be cut with a knife), excellent conductors of electricity, etc.

17
Q

State the periodic law.

A

The physical and chemical properties of elements are periodic functions of their atomic numbers.

18
Q

What is another name for the main group elements?

A

______representative elements__________________

19
Q

What is a semiconductor?

A

A crystalline material with intermediate electrical conductivity

20
Q

Name the scientist who revised the periodic table to give us the table that we use today. How did he change Mendeleev’s table?

A

Mosely; Arranged it by atomic number instead.

21
Q

List the metalloids.

A

B, Si, Ge, As, Sb, Te

22
Q

Half the distance between two atoms bonded together

A

bond radius

23
Q

Metallic character ( increases / decreases ) as you move from left to right across the periodic table.

A

decreases

24
Q

High / Low ) ionization energy means that electrons are difficult to remove.

A

High

25
Q

( More negative / Less negative ) electron affinity means that electrons are more strongly attracted to the atom.

A

more negative

26
Q
  1. List four properties of halogens.
A

Combine with metals to produce salts, most reactive nonmetals, seven electrons in outer E level, often acquire one e- in chemical reactions to form -1 ions

27
Q

Half the distance between two adjacent, nonbonded nuclei is called

A

van der waals radius

28
Q
  1. List four properties of noble gases.
A

Not reactive, full outer energy level (stable octet), all gases, don’t bond with other elements, mostly inert, used in illuminated signs (Ne and Ar)

29
Q

List four properties of alkaline earth metals.

A

Harder, denser, stronger, and have higher melting points than alkali metals; reactive, but not as much as alkali metals; have two electrons in outer energy level

30
Q
  1. What are salts formed from?
A

a halogen and a metal

31
Q

List four properties of metals.

A

Malleability (bendability), ductility (can be pulled into a wire), conduct heat, conduct electricity, luster (shiny)

32
Q

Explain what “electron shielding” is.

A

The reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charge of the other (core) electrons.