Chem Chapter 6 Test

Question 1

In electron dot structure which element could X represent?

Answer 1

Chlorine

Question 2

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

Answer 2

Increases

Question 3

The greatest absorbtion of energy occurs from electron moves from

Answer 3

1s to 3s

Question 4

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

Answer 4

n=1

Question 5

What principle energy level can hold a max of 18 electrons

Answer 5

3 (2n^2)

Question 6

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

Answer 6

2-8-18-18-1

Question 7

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

Answer 7

2-8

Question 8

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?

Answer 8

2-8-18-18-2

Question 9

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

Answer 9

s and p sub levels only

Question 10

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

Answer 10

The electron config that adds up to 6

Question 11

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

Answer 11

Period 3 Group 16

Question 12

Which electron config represents an electron in its excited state?

Answer 12

The electron config that jumps around

Question 13

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

Answer 13

1s2 2s2 2p2 3s1

Question 14

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

Answer 14

9

Question 15

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

Answer 15

4

Question 16

What principle energy level has no f sub level?

Answer 16

3

Question 17

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

Answer 17

2

Question 18

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

Answer 18

6

Question 19

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

Answer 19

Oxygen

Question 20

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

Answer 20

3s electrons

Question 21

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

Answer 21

6 electrons

Question 22

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)

Answer 22

7

Question 23

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

Answer 23

The one completely filled

Question 24

In the modern Periodic Table elements are arranged by what?

Answer 24

Atomic Number

Question 25

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

Answer 25

An alkali Metal

Question 26

Which two elements have the most similar chemical properties?

Answer 26

Which ever elements is right below the other

Question 27

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

Answer 27

Larger nucleus charge

Question 28

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

Answer 28

Whichever one is closest to the top right

Question 29

Which has the largest atomic radius?

Answer 29

Whichever one is closest to the bottom left

Question 30

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

Answer 30

Increase and the ionization decreases

Question 31

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

Answer 31

The relative electronegativity increases and the atomic radius decreases

Question 32

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

Answer 32

fewer electrons

Question 33

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

Answer 33

larger radius and more electrons

Question 34

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

Answer 34

Metals

Question 35

``` Which element is considered malleable? Gold Radon Hydrogen Sulfur ```

Answer 35

Gold

Question 36

Which element has the most pronounce metallic prop

Answer 36

The one closest to the bottom left

Question 37

Which period 3 element has the least metallic characteristic

Answer 37

The one farthest from the bottom left

Question 38

``` 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? ```

Answer 38

C

Question 39

A non-metal could have an electronegitivity of

Answer 39

2.6

Question 40

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

Answer 40

Be brittle

Question 41

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

Answer 41

Non-metal, metalloid, metal

Question 42

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

Answer 42

Ionization Energy

Question 43

The highest ionization energies are found in group what?

Answer 43

18

Question 44

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

Answer 44

(F) or the closest one to the Noble Gases

Question 45

Which atom will lose an electron most readily?

Answer 45

The ones closest to the bottom left

Question 46

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

Answer 46

larger nuclear energy

Question 47

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

Answer 47

MCl

Question 48

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

Answer 48

1

Question 49

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

Answer 49

2

Question 50

Which aqueous salt solution has a color?

Answer 50

CuSO4(aq)

Question 51

--------> =

Answer 51

Period

Question 52

``` | | | | \/ ```

Answer 52

Group

Question 53

Ionization Rule

Answer 53

``` Larger= Top Right Lower= Bottom Left ```

Question 54

Radius Rule

Answer 54

``` Larger= Bottom Left Lower= Top Right ```

Question 55

0-2 is a

Answer 55

Metal

Question 56

2 is a

Answer 56

Metalloid

Question 57

More than 2 is a

Answer 57

Non-Metal

Question 58

Periodic Law

Answer 58

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

Question 59

Metals

Answer 59

Are generally good conductors of heat and electric current

Question 60

Non metals

Answer 60

Poor conductors of heat and electric Currents

Question 61

Metalloids

Answer 61

Generally has properties similar to those of metals and non metals

Question 62

Alkali Metal

Answer 62

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

Question 63

Alkali Earth Metals

Answer 63

Elements in group 2A

Question 64

Halogens

Answer 64

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

Question 65

What Elements are the most like halogens?

Answer 65

Salt, Chlorine, Bromine, and Iodine

Question 66

Noble Gases

Answer 66

Elements in Group 8A on the Periodic Table

Question 67

Representative Elements

Answer 67

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

Question 68

Transition Metals

Answer 68

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

Question 69

Inner Transition Metals

Answer 69

Elements that appear below the main body of the periodic table

Question 70

Atomic Radius

Answer 70

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

Question 71

Ion

Answer 71

Atom or group of atoms with a positive and negative charge

Question 72

Cation

Answer 72

Ion with a positive Charge

Question 73

Anion

Answer 73

Ion that is negatively charged

Question 74

Ionization Energy

Answer 74

Energy required to remove an electron from an atom

Question 75

Electronegitvity

Answer 75

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

Question 76

Electron Affinity

Answer 76

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

Question 77

Diatomic Elements

Answer 77

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