4, 5, 6 Test

Question 1

The sum of these subatomic particles equal the atomic number

Answer 1

protons

Question 1

An equal numbers of these particles results in a neutral atom

Answer 1

protons and electrons

Question 2

A gain of these creates an anion

Answer 2

electrons

Question 3

This particle is located outside the nucleus

Answer 3

electrons

Question 4

A change in these particles changes the identity of the element

Answer 4

protons

Question 5

The majority of the mass of the atom is contributed by these particles

Answer 5

protons and neutrons

Question 6

These particles are neutral

Answer 6

neutrons

Question 7

Which color would possess the lowest energy?

Answer 7

red

Question 8

Which color would have the shortest wavelength?

Answer 8

blue

Question 9

The cathode ray is composed of

Answer 9

electrons

Question 10

According to this principle, the 2s orbital must be filled before the 2p orbital

Answer 10

Aufbau

Question 11

Which orbital is impossible to exist according to quantum mechanics?

Answer 11

1p

Question 12

Nitrogen is located in which block?

Answer 12

p

Question 13

If isotope A has a mass of 5.0 grams and isotope B has a mass of 6.0 grams and both contain the same number of protons, and there are only two isotopes both of which contain 50% of abundance. Calculate the average atomic mass

a) 5.25 amu
b) 5.60 amu
c) 5.75 amu
d) none of these

Answer 13

none of these

Question 14

The last two electrons of CI are located in which orbital?

Answer 14

p

Question 15

How many electrons does a subshell of f orbitals contain?

Answer 15

14

Question 16

Which element contains 2 protons?

Answer 16

helium

Question 17

He conducted the gold foil experiment

Answer 17

Rutherford

Question 18

He proposed the plum-putting model

Answer 18

Thomson

Question 19

This was the first scientist to propose that atoms form compounds in simple whole number ratio

Answer 19

Dalton

Question 20

He discovered the nucleus of the atom

Answer 20

Rutherford

Question 21

He first proposed that the atom is composed of positive and negative charges

Answer 21

Thomson

Question 22

He showed that electrons orbit the nucleus at specific energy levels

Answer 22

Bohr

Question 23

He first demonstrated that most of the atom’s volume consists of the electron cloud

Answer 23

Rutherford

Question 24

Which quantum number, represents the subshell of an atom

Answer 24

angular momentum

Question 25

What is the ratio of mass of sulfur to the mass of oxygen in the molecule SO

Answer 25

2:1

Question 26

Which is false concerning the conversion of hydrogen peroxide to oxygen and hydrogen gas? [H2O2 --> O2 +H2]

Answer 26

The mass of hydrogen atoms in peroxide is less than the mass of hydrogen in hydrogen gas

Question 27

The energy level of the outermost electrons of vanadium is located in the

Answer 27

fourth

Question 28

What element is represented by the [Ar] 4s2 3d1

Answer 28

scandium

Question 29

Which of the following orbital is at the highest energy level

Answer 29

4f

Question 30

A positive ion is a

Answer 30

caltion

Question 31

how many electrons does the first energy level contain?

Answer 31

2

Question 32

Group 1 and 2 (alkaline and alkali earth metals respectively) are part of the

Answer 32

s block

Question 33

What is the correct order that orbitals must be filled

Answer 33

1s--> 2s --> 2p --> 3s --> 3p --> 4s --> 3d --> 4p

Question 34

How many electrons does a neutral atom of sodium ion contain?

Answer 34

11

Question 35

Which orbital is shaped like a sphere?

Answer 35

s

Question 36

The elements of the fourth period of the periodic table contain which subshells?

Answer 36

s & p & d

Question 37

The lowest state of energy an atom is its

Answer 37

ground state

Question 38

Which subatomic particles are not held by nuclear forces?

Answer 38

protons and electrons

Question 39

This property results in a cation

Answer 39

ionization energy

Question 40

The energy required to remove an electron from a neutral atom

Answer 40

ionization energy

Question 41

This property increases down a group and decreases across a period

Answer 41

atomic radius (atomic size)

Question 42

The measure of the ability of an atom to attract an electron in a chemical compound

Answer 42

electronegativity

Question 43

He proposed moving the lanthanides and the actinides from the main body of the periodic table

Answer 43

Seaborg

Question 44

He grouped elements into triads

Answer 44

Dobereiner

Question 45

He proposed the law of octaves

Answer 45

Newlands

Question 46

He arranged the periodic table according to increasing atomic number

Answer 46

Moseley

Question 47

Both of these scientists arranged elements according to increasing atomic mass

Answer 47

Mendeleev and Meyer

Question 48

These elements are not included as part of the main group elements

Answer 48

transition elements

Question 49

These elements rarely form compounds

Answer 49

noble gases

Question 50

This group loses two electrons

Answer 50

akkalune earth metals

Question 51

These are the most reactive of the nonmetals

Answer 51

halogens

Question 52

Which element has more metallic character

Answer 52

Sulfur

Question 53

Which element is smaller

Answer 53

Fluorine

Question 54

Which element has a lower electronegativity

Answer 54

Sodium

Question 55

Which element has a larger radius

Answer 55

Francium

Question 56

Which element has a stronger electron affinity

Answer 56

Carbon

Question 57

Which metal is the most reactive

Answer 57

Potassium

Question 58

Which nonmetal is the most reactive

Answer 58

Fluorine

Question 59

Explain why smaller atoms have greater ionization energies

Answer 59

The electrons are being held in closer to the protons, which have opposing charges and therefore hold on to them, in an atom with a small radius

Question 60

Smaller atoms have lower negativity than larger atoms. If helium is the smallest atom, why is fluorine identified as the element with the greatest electronegativity?

Answer 60

It can strongly attract a shared pair of electrons toward itself