Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

DAT GenChem > GenChem2 (PeriodicTable) > Flashcards

GenChem2 (PeriodicTable) Flashcards

1
Q

Periodic Law states that the chemical properties of the elements are dependent, in a systematic way, upon their

A

Atomic numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

How many periods (rows) are there?

A

7

They represent n=1 to n=7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Groups represent elements that have the same electronic configuration in their _____, and the have similar chemical properties because of it

A

Valence Shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

The Roman numeral above each group represents the number of

A

Valence Electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

A groups have ____ sublevels as their outermost orbitals

B groups have _____ sublevels as their outermost orbitals

A

s and p

d and f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

The B elements include these groups

A

transition elements
lanthanide series
actinide series

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

This B element group has partially filled d levels

A

Transition elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

This B element has partially filled f sublevels

A

Lanthanide and Actinide Series

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING/DECREASING amount of nuclear attraction

A

As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING amount of nuclear attraction
(they become closer and more tightly bound to the nucleus)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

As one goes down a column, the outermost electrons become MORE/LESS tightly bound to the nucleus

A

As one goes down a column, the outermost electrons become LESS tightly bound to the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

The _____ is equal to one-half the distance between the centers of two atoms of that element that are just touching each other

A

Atomic radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Atomic radius ______ from right to left and ________ down a given group

A

Atomic radius decreases from right to left and increases down a given group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

The atoms with the largest atomic radius will be located where on the periodic table?

A

Bottom of group 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

The energy required to completely remove an electron from a gaseous atom or ion.

A

Ionization Energy (IE) or Ionization Potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Is removing an electron exothermic or endothermic?

A

Endothermic, as it requires energy.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

The energy required to remove one valence electron from the parent atom

The energy required to remove a second valence electron from the univalent ion to form the divalent ion

A

Second Ionization energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Which has a greater ionization energy, second or first ionization energy?

A

second ionization energy

IEs grow increasingly large

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

From left to right across the periodic table, ionization energy INCREASES/DECREASES

Why?

A

From left to right across the periodic table, ionization energy INCREASES

The atomic radius DECREASES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Moving down a group, ionization energy INCREASES/DECREASES

Why?

A

Moving down a group, ionization energy DECREASES

The atomic radius increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Defined as the energy change that occurs when an electron is added to a gaseous atom, and represents the ease to with which the atom can accept an electron.

A

Electron Affinity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Positive electron affinity (in this text) represents energy absorption when an electron is added or energy release?

A

Energy release

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Group IIA elements have HIGH/LOW electron affinityies

Group VIIA elements have HIGH/LOW electron affinities

A

Group IIA elements have LOW electron affinityies

Group VIIA elements have HIGH electron affinities

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

A measure of the attraction an atom has for electrons in a chemical bond

A

Electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Electronegativities are related to…

A

Ionization energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Electrons with low ionization energies have HIGH/LOW electronegativities

Why?

A

Electrons with low ionization energies have LOW electronegativities

Their nuclei do not strongly attract electrons.

26
Q

Electrons with high ionization energies have HIGH/LOW electronegativities

Why?

A

Electrons with high ionization energies have HIGH electronegativities

The nucleus has a strong pull on the electrons

27
Q

As you move from left to right across the periodic table, electronegativity ______

As you increases the atomic number in a group, electronegativity ______

A

Increases

Decreases because of increased distance between valence shell and nucleus

28
Q

The three categories of elements in the periodic table

A

Nonmetals, Metals, Metalloids

29
Q

Category of elements that have high densities and high melting points, and are solid at room temperature

A

Metals

30
Q

Metalshave the ability to be deformed without breaking, like hammering it into different shapes. This characteristic ability of metals is called

A

Malleability

31
Q

The ability of metal to be drawn into a wire

A

Ductility

32
Q

Metals have a SMALL/LARGE atomic radius
Metals have a HIGH/LOW IE
Metals have a HIGH/LOW electronegativity

These properties are explained by

A

Metals have a LARGE atomic radius
Metals have a LOW IE
Metals have a LOW electronegativity

These properties are explained by the few electrons in the valence shell which can be easily removed.

33
Q

Metals are BAD/GOOD conductors of electricity and heat?

Why?

A

Metals are GOOD conductors of electricity and heat

The valence electrons can move freely

34
Q

Which metals are the most reactive metals?

A

Groups IA and IIA

35
Q

This category of elements is brittle in the solid state and show little or no metallic luster.

A

Nonmetals

36
Q

Nonmetals have HIGH/LOW IE
Nonmetals have HIGH/LOW electronegativit
Nonmetals are GOOD/POOR conductors of heat and electricity

A

Nonmetals have HIGH ionization energies
Nonmetals have HIGH electronegativity
Nonmetals are POOR conductors of heat and electricity (usually)

37
Q

Name the one characteristic of nonmetals that they share, otherwise they have a wide range of chemical behaviors and reactivities

A

Nonmetals share the ability to gain electrons easily

38
Q

The category of elements located along the line between the metals and nonmetals on the periodic table

A

Metalloids

39
Q

Are metalloid properties universal or diverse?

A

Their properties vary considerably

Densities, BPs, and MPs

40
Q

Metalloids have HIGH/LOW/INTERMEDIATE electronegativites and IEs

A

Intermediate between metals and nonmetals, they possess characteristics of both classes

41
Q

What does the reactivity of metalloids depend pon?

A

The element with which they are reacting

42
Q

B behaves as a nonmetal when reacting with…

B behaves as a metal when reacting with…

A

Na

F

43
Q

Name the elements classified as metalloids

A

Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium

44
Q

The elements of group IA are referred to as

A

Alkali Metals

45
Q

How do alkali differ from other metals?

Why?

A

They have lower densities.

They have one loosely bound electron in the valence shell, meaning they have the largest atomic radii in a period.

46
Q

Alkali metals have ____ IEs
Alkali metals have ____ electronegativity
Alkali metals have _____ reactivity

Why?

A

Low IEs
Low electronegativity
High reactivity

They easily lose their valence electron

47
Q

What group do alkali metals react easily with? Especially…

A

Nonmetals, especially halogens

48
Q

The elements of group IIA are the…

A

Alkaline earth metals

49
Q

Alkaine earths have a LARGER/SMALLER atomic radius than alkali metals

A

Smaller.

50
Q

Can the two valence electrons of alkaline earths be removed to form divalent cations?

A

Yes.

51
Q

Alkaline earths have _____ IEs

Alkaline earths have _____ electron affinities

A

Alkaline earths have LOW IEs

Alkaline earths have LOW electron affinities

52
Q

Elements in group VIIA are the…

A

Halogens

53
Q

Halogens have ____ reactivity

Why?

A

Halogens have HIGH reactivity

Seven electrons in the valence shell

54
Q

In terms of physical properties, are the halogens uniform or diverse?

A

Halogens are highly variable.

F2 and CL2 are gaseous, Br2 is liquid, I2 is solid at room temperature

55
Q

Are the chemical properties of halogens uniform or diverse?

What group of elements are halogens most reactive with?

A

Uniform.

High electronegativities, high ionization energies

Alkali Metals and Alkaline Earth metals (group IA and IIA)

56
Q

The group of elements found in group VIIIA are the…

A

Noble Gases

57
Q

The noble gases are REACTIVE/NONREACTIVE
The noble gases have HIGH/LOW IEs
The noble gases have HIGH/LOW electronegativities

Why?

A

NONREACTIVE
HIGH IEs
NO ELECTRONEGATIVITIES

Noble gases have a full valence shull

58
Q

Groups IB to VIIIB are the

A

Transition metals.

59
Q

The transition metals are very SOFT/HARD
The transition metals have HIGH/LOW melting points
Transition elements have HIGH/LOW IEs

A

The transition metals are very HARD
The transition metals have HIGH BPs
The transition metals have LOW IEs

60
Q

Transition metals may exist in a variety of positively charged forms, aka

Why?

A

Oxidation states

Transition metals are capable of losing various numbers of electrons from the s and d orbitals of the valence shell

61
Q

Dissolves ions of transition metals can form ____ with other molecules of water or with nonmetals

Does the formation of complex ions increase or decrease the solubility of a compound?

A

Complex Ions

It enhances the solubility

62
Q

What gives the complex ions their characteristic colors?

A

The d orbitals split into two energy sublevels, enabling complexes to absorb certain frequencies of light. Those not absorbed are observed.

DAT GenChem (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions