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Chemistry 2013-2014 > Chem Chapter 6 Test > Flashcards

Chem Chapter 6 Test Flashcards

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1
Q

In electron dot structure which element could X represent?

A

Chlorine

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2
Q

As an electron from ground state to excited state the potential energy of the atom

A

Increases

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3
Q

The greatest absorbtion of energy occurs from electron moves from

A

1s to 3s

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4
Q

What principle energy level of an atom contains an electron with the lowest energy

A

n=1

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5
Q

What principle energy level can hold a max of 18 electrons

A

3 (2n^2)

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6
Q

If the electron config for silver is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10 what is the configuration for the ground state of the silver

A

2-8-18-18-1

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7
Q

If the electron configuration for Mg is 1s2 2s2 2p6 3s2 what is the configuration for Mg+2

A

2-8

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8
Q

If the electron config for silver is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10 which represents the electron configuration of a silver ion (Ag+) in the ground state?

A

2-8-18-18-2

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9
Q

Four valance electron on an atom in the ground state would occupy the

A

s and p sub levels only

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10
Q

Which of the following is the electron config of a neutral atom in the ground state with a total of six valance electrons

A

The electron config that adds up to 6

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11
Q

Given the electron config of an atom in the ground state 1s2 2s2 2s6 3s2 3p4 This element is found in the periodic table

A

Period 3 Group 16

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12
Q

Which electron config represents an electron in its excited state?

A

The electron config that jumps around

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13
Q

Which electron config is possible for a nitrogen atom in its excited state (Nitrogen electron config is 1s2 2s2 2p3)

A

1s2 2s2 2p2 3s1

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14
Q

What is the total number of orbitals in the third principle energy level?

A

9

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15
Q

What is the total number of occupied s orbitals in a atom of nickle in its ground state

A

4

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16
Q

What principle energy level has no f sub level?

A

3

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17
Q

The maximum number of electrons that a single orbital of the 3d sublevel may contain is

A

2

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18
Q

A neutral atom of an element has an electron configuration of 2-8-2. What is the total number of p electrons in this atom

A

6

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19
Q

Which atom in the ground state contains 1 completely filled orbital?

A

Oxygen

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20
Q

A Sulfur atom and a chlorine atom have the same number of

A

3s electrons

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21
Q

A neutral atom in the ground state contains 16 electrons. What is the total number of electrons in the 2p sublevel

A

6 electrons

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22
Q

What are the total number of sub levels that that contain electrons in an atom of zinc in the ground state (1s2 2s2 2p6 3s2 3p6 4s2 3d10)

A

7

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23
Q

Which orbital notation represents the second principle energy level of a silicon atom in the ground state (1s2 2s2 2p6 3s2 3p2)

A

The one completely filled

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24
Q

In the modern Periodic Table elements are arranged by what?

A

Atomic Number

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25
Q

An atom of an element contains 20 protons, 20 neutrons and 20 electrons, This element is

A

An alkali Metal

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26
Q

Which two elements have the most similar chemical properties?

A

Which ever elements is right below the other

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27
Q

Compare the atomic radius of a sodium atom, the atomic radius of a magnesium is smaller. The radius is primarily a result of the magnesium having a

A

Larger nucleus charge

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28
Q

According to the periodic table which element has the smallest atomic radius?

A

Whichever one is closest to the top right

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29
Q

Which has the largest atomic radius?

A

Whichever one is closest to the bottom left

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30
Q

As the element of group 16 are considered from top to bottom on the periodic table the atom radii

A

Increase and the ionization decreases

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31
Q

As the elements Li to F in period 2 are considered in succession, how do the relative electronegativity and atomic radius of each successive element compare

A

The relative electronegativity increases and the atomic radius decreases

32
Q

The radius of a calcium ion is smaller than the radius of a calcium atom because the calcium ion contains the same nuclear charge and

A

fewer electrons

33
Q

The S2- ion differs from the S0 atom in that the S2- ion has a

A

larger radius and more electrons

34
Q

More than two thirds of the elements in the periodic table are

A

Metals

35
Q 
Which element is considered malleable?
Gold
Radon
Hydrogen 
Sulfur
A

Gold

36
Q

Which element has the most pronounce metallic prop

A

The one closest to the bottom left

37
Q

Which period 3 element has the least metallic characteristic

A

The one farthest from the bottom left

38
Q 
The Table below shows some properties of elements A, B, C, D
Element     IE     EN     COHAE
A             Low   Low        Low
B             Low   Low        High
C             High  High       Low
D             High  High       High 
IE= Ionization Energy
EN= Electronegativity 
COHAE= Conductor of Heat and Electricity 
What element is most likely non-metal?
A

C

39
Q

A non-metal could have an electronegitivity of

A

2.6

40
Q

Non-metals in the solid state are poor conductors of heat and tend to

A

Be brittle

41
Q

As elements are considered from top to bottom in Group 15 which sequence in properties occur

A

Non-metal, metalloid, metal

42
Q

The amount of energy required to remove the most loosely bound electron from an atom in the gaseous state is called

A

Ionization Energy

43
Q

The highest ionization energies are found in group what?

A

18

44
Q

Which element in group 2 has the greatest tendency to gain electrons

A

(F) or the closest one to the Noble Gases

45
Q

Which atom will lose an electron most readily?

A

The ones closest to the bottom left

46
Q

A reason why chlorine has a high ionization energy than sulfur is that chlorine has a

A

larger nuclear energy

47
Q

If M represents an atom of an alkali metal, the correct formula for a compound of this atom with chlorine is

A

MCl

48
Q

Which group of elements occur only as compounds in nature because they are extremely reactive

A

1

49
Q

What group in the periodic table contains the elements of the alkaline earth family

A

2

50
Q

Which aqueous salt solution has a color?

A

CuSO4(aq)

51
Q

——–> =

A

Period

52
Q 
|
 |
 |
 |
\/
A

Group

53
Q

Ionization Rule

A 
Larger= Top Right 
Lower= Bottom Left
54
Q

Radius Rule

A 
Larger= Bottom Left
Lower= Top Right
55
Q

0-2 is a

A

Metal

56
Q

2 is a

A

Metalloid

57
Q

More than 2 is a

A

Non-Metal

58
Q

Periodic Law

A

When elements are arranged in order of increasing atomic Number, there is a repetition of their physical and chemical properties

59
Q

Metals

A

Are generally good conductors of heat and electric current

60
Q

Non metals

A

Poor conductors of heat and electric Currents

61
Q

Metalloids

A

Generally has properties similar to those of metals and non metals

62
Q

Alkali Metal

A

Elements in group 1A (comes from Arabic word “al aqali” meaning “the ashes”)

63
Q

Alkali Earth Metals

A

Elements in group 2A

64
Q

Halogens

A

Nonmetal group 7A (Combination of Greek Words “hals” meaning “Salt” And Latin word “genesis” meaning “to be born”)

65
Q

What Elements are the most like halogens?

A

Salt, Chlorine, Bromine, and Iodine

66
Q

Noble Gases

A

Elements in Group 8A on the Periodic Table

67
Q

Representative Elements

A

Elements in Groups 1A to Group 7A are often referred to as Transition Metals because they display a wide range of physical and chemical properties

68
Q

Transition Metals

A

Group B elements that are usually displayed int eh main body part of the periodic table

69
Q

Inner Transition Metals

A

Elements that appear below the main body of the periodic table

70
Q

Atomic Radius

A

One half of the distance between the nuclei of two atoms of the same element when the atoms are joined

71
Q

Ion

A

Atom or group of atoms with a positive and negative charge

72
Q

Cation

A

Ion with a positive Charge

73
Q

Anion

A

Ion that is negatively charged

74
Q

Ionization Energy

A

Energy required to remove an electron from an atom

75
Q

Electronegitvity

A

Ability of an atom of an element to attract electrons when the atom is in a compound

76
Q

Electron Affinity

A

The energy change by a gaseous atom or ion to gain an electron

77
Q

Diatomic Elements

A 
Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Fluorine (F2)
Chlorine (Cl2)
Iodine (I2)
Bromine (Br2)

Chemistry 2013-2014 (20 decks)

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