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Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

States that when the elements are arranged in order of increasing atomic number, elements with similar properties fall into the same groups.

A

The Periodic Law

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2
Q

Another name for the top row of the f-block of elements

A

The lanthanides

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3
Q

Another name for the bottom row of the f-block of elements.

A

The actinides

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4
Q

The entire f-block of elements is also sometimes referred to as this.

A

The inner transition metals

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5
Q

The name for a vertical column of elements on the periodic table.

A

A group

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6
Q

The name for a horizontal row of elements on the periodic table.

A

A period

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7
Q

The type of elements that separate the metals (to the left) from the non-metals (to the right).

A

The metalloids

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8
Q

The s-block of elements includes these groups.

A

IA and IIA

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9
Q

The p-block of elements includes these groups.

A

IIIA through VIIIA

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10
Q

The s-block and p-block of elements are collectively known as this.

A

The main group elements

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11
Q

The d-block of elements includes these groups.

A

IIIB through IIB

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12
Q

The d-block of elements is commonly called by this name.

A

The transition metals

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13
Q

Which element is placed with the p-block elements, but does not really belong with these elements?

A

Helium

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14
Q

What does an an element’s block indicate about its electron configuration?

A

The block tells the last filling sublevel for an element

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15
Q

What is another name for the group IA (1A) elements (except hydrogen)?

A

The alkali metals

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16
Q

What is another name for the group IIA (2A) elements?

A

The alkaline earth metals

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17
Q

What is another name for the group VIIA (7A) elements?

A

The halogens

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18
Q

What is another name for the group VIIIA (8A) elements?

A

The noble gases

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19
Q

Rank the following metals in order of increasing hardness (softest first): aluminum, sodium, iron. Explain your answer.

A

Sodium, aluminum, iron. In general, s-block metals are the softest, followed by p-block metals, and d-block metals tend to be the hardest.

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20
Q

How can the last filling sublevel for an s-block or p-block element be predicted by looking at the periodic table?

A

Let n = the period in whch the element is found. Then the last filling sublevel for an s-block element is ns. The last filling sublevel for a p-block element is np.

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21
Q

How can the last filling sublevel for a d-block element be predicted by looking at the periodic table?

A

Let n = the period in which the element is found. Then the last filling sublevel for a d-block element is (n-1)d.

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22
Q

How can the last filling sublevel for a f-block element be predicted by looking at the periodic table?

A

Let n = the period in which the element is found. Then the last filling sublevel for a f-block element is (n-2)f.

23
Q

One half the distance between the nuclei of identical atoms that are bonded together.

A

Atomic radius

24
Q

What is the general trend for atomic radius across a period. Why?

A

Atomic radius tends to decrease across a period. Going across a period (for main group elements), more protons are added to the nucleus, as more valence electrons are added. The number of core electrons stays the same, so no extra shielding occurs. As a result, the valence electrons are pulled more tightly to the nucleus.

25
Q

What is the general trend for atomic radius down a group? Why?

A

Going down a group, atomic radius tends to increase. Moving down a group, electrons are being added to the next higher energy level. Orbitals of higher energy levels are larger than those of lower energy levels. The electrons in the higher energy levels are farther from the nucleus.

26
Q

An atom that has gained or lost one or more electrons.

A

An ion

27
Q

A positively charged ion that results from a metal losing one or more electrons.

A

A cation

28
Q

A negatively charged ion that results from a non-metal gaining one or more electrons.

A

An anion

29
Q

The energy required to remove an electron from a neutral atom in the gaseous state.

A + energy –> A+1 + e-

A

Ionization energy

30
Q

What is the trend for ionization energies across a period of elements? Why?

A

Ionization energies tend to increase across a period. The atoms to the right are smaller, so their valence electrons are closer to the nucleus and held more tightly. Therefore it requires more energy to remove an electron from atoms to the right of a given period.

31
Q

What is the trend for ionization energy down a group of the periodic table?

A

Ionization energy tends to decrease down a group. The atoms at the bottom of a group are the larger, and their valence electrons are farther from the nucleus, and are held less tightly. Therefore the valence electrons of bigger atoms require less energy to remove, so the atoms at the bottom of a given group have lower ionization energies.

32
Q

Why is there a large increase from 1st to 2nd ionization energy for the group IA elements?

A

The group IA elements have one valence electron. This electron is farther from the nucleus than the core electrons, and is easier to remove. Core electrons tend to be closer to the nucleus and are held more tightly. Removing a second electron from a group IA element means taking away one of these more tightly held core electrons, requiring significantly more energy.

A similar phenomenon occurs for atoms in other groups. For example, there is a large jump from the 2nd to 3rd ionization energy for the group IIA elements (the 2 valence electrons are easier to remove than the third electron, which would come from the core).

33
Q

Which has a greater radius: an atom or its cation? Why?

A

The radius of an atom is always larger than that of its cation. After removing an electron to form an cation, there is less repulsion present among the remaining electrons, so the radius decreases. Additionally, metals tend to lose all valence electrons when forming cations. This empties out the highest energy level, leaving only the core electrons in the lower energy levels (with smaller orbitals).

34
Q

Which is larger: an atom or its anion? Why?

A

An anion is always larger than its atom. Adding extra electrons increases the amount of electron-electron repulsion, making the anion’s radius expand. The charge of the nucleus remains the same, so there is no additional attractive force to pull in the extra electrons.

35
Q

What is the period trend for the radii of cations? For anions? Why?

A

Both cations and anions grow smaller across a period for the same reason that atomic radius decreases across a period (increasing effective nuclear charge).

36
Q

What is the group trend for the radii of cations? For anions? Why?

A

Both cations and anions grow larger down a group for the same reason that atomic radius increases down a group (electrons are in higher energy levels, farther from the nucleus).

37
Q

Ionic radius tends to decrease across a period. Why is there a sharp increase in ionic radius followed by another decrease in ionic radius towards the right of every period of elements?

A

The sharp increase in radius corresponds to the last cation in the period and fist anion in that period.

38
Q

Electrons in the highest energy level of an atom are called….

A

Valence electrons

39
Q

The energy change that occurs when an electron is acquired by a neutral atom in the gaseous state.

A

Electron affinity

40
Q

What is the trend down a group for electron affinity? Why?

A

Electron affinity tends to decrease (become less negative) down a group. The atoms at the bottom of a group are larger, and their nuclei are in the center of a larger electron cloud, making it more difficult for the nucleus to attract extra electrons. There a numerous exceptions to this trend.

41
Q

Which is the last sublevel to fill for each of the following elements? Why?

Radium (Ra)

Tellurium (Te)

Osmium (Os)

Uranium (U)

A

Radium (Ra) - 7s; last sublevel to fill for an s-block element is the ns sublevel

Tellurium (Te) - 5p; last sublevel to fill for a p-block element is the np sublevel

Osmium (Os) - 5d; last sublevel to fill for a d-block element is the (n-1)d sublevel

Uranium (U) - 4f; last sublevel to fill for an f-block element is the (n-2)f sublevel

42
Q

How many valence electrons does an atom of each of the following elements have? Why?

Beryllium (Be)

Silicon (Si)

Polonium (Po)

A

Beryllium (Be) - 2

Silicon (Si) - 4

Polonium (Po) - 6

For the main group elements, the group number tells the number of valence electrons.

43
Q

What is the highest overall occupied energy level for an atom of each of the following elements?

Lanthanum (La)

Nitrogen (N)

Plutonium (Pu)

Potassium (K)

A

Lanthanum (La) - 6

Nitrogen (N) - 2

Plutonium (Pu) - 7

Potassium (K) - 4

For any element, the highest overall occupied energy level is equal to the period number.

44
Q

For the following elements, state the period and the group to which each element belongs.

[Ar]3d104s24p3

[Kr]5s1

[Xe]5d36s2

A

[Ar]3d104s24p3 - Group VA, Period 4 (As)

[Kr]5s1 - Group IA, Period 5 (Rb)

[Xe]5d36s2 - Group VB, Period 6 (Ta)

45
Q

Arrange the following elements in order of expected increasing atomic radius (smallest first):

Xe, Ne, Ar

A

Ne, Ar, Xe

Atomic radius increases down a group

46
Q

Arrange the following elements in order of expected increasing atomic radius (smallest first):

Ba, Bi, Tl

A

Bi, Tl, Ba

Atomic radius decreases across a period

47
Q

Arrange the following elements in order of expected ionization energy (smallest first):

Ca, K, Br

A

K, Ca, Br

Ionization energy increases across a period

48
Q

Arrange the following elements in order of expected ionization energy (smallest first):

Sn, Pb, C

A

Pb, Sn, C

Ionization energy decreases down a group

49
Q

Which of the following would be expected to have the most negative electron affinity?

At, I, Br

A

Bromine. Electron affinity tends to become less negative down a group.

50
Q

Arrange the following elements in order of expected increasing ionic radius (smallest first):

Al+3, In+3, Ga+3

A

Al+3, Ga+3, In+3

ionic radius tends to increase down a group.

51
Q

Arrange the following elements in order of expected increasing ionic radius (smallest first):

S-2, Cl-1, P-3

A

Cl-1, S-2, P-3

Ionic radius tends to decrease across a period

52
Q

Which is the larger in the pair?

Sr or Sr+2?

A

Sr. An atom is always bigger than its cation

53
Q

Which is the larger in the pair?

Br or Br-1

A

Br-1. An anion is always larger than its atom

Chemistry (13 decks)

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