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Chem Honors > 4, 5, 6 Test > Flashcards

4, 5, 6 Test Flashcards

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1
Q

The sum of these subatomic particles equal the atomic number

A

protons

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1
Q

An equal numbers of these particles results in a neutral atom

A

protons and electrons

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2
Q

A gain of these creates an anion

A

electrons

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3
Q

This particle is located outside the nucleus

A

electrons

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4
Q

A change in these particles changes the identity of the element

A

protons

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5
Q

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

A

protons and neutrons

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6
Q

These particles are neutral

A

neutrons

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7
Q

Which color would possess the lowest energy?

A

red

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8
Q

Which color would have the shortest wavelength?

A

blue

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9
Q

The cathode ray is composed of

A

electrons

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10
Q

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

A

Aufbau

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11
Q

Which orbital is impossible to exist according to quantum mechanics?

A

1p

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12
Q

Nitrogen is located in which block?

A

p

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13
Q

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

A

none of these

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14
Q

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

A

p

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15
Q

How many electrons does a subshell of f orbitals contain?

A

14

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16
Q

Which element contains 2 protons?

A

helium

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17
Q

He conducted the gold foil experiment

A

Rutherford

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18
Q

He proposed the plum-putting model

A

Thomson

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19
Q

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

A

Dalton

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20
Q

He discovered the nucleus of the atom

A

Rutherford

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21
Q

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

A

Thomson

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22
Q

He showed that electrons orbit the nucleus at specific energy levels

A

Bohr

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23
Q

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

A

Rutherford

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24
Q

Which quantum number, represents the subshell of an atom

A

angular momentum

25
Q

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

A

2:1

26
Q

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

A

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

27
Q

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

A

fourth

28
Q

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

A

scandium

29
Q

Which of the following orbital is at the highest energy level

A

4f

30
Q

A positive ion is a

A

caltion

31
Q

how many electrons does the first energy level contain?

A

2

32
Q

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

A

s block

33
Q

What is the correct order that orbitals must be filled

A

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

34
Q

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

A

11

35
Q

Which orbital is shaped like a sphere?

A

s

36
Q

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

A

s & p & d

37
Q

The lowest state of energy an atom is its

A

ground state

38
Q

Which subatomic particles are not held by nuclear forces?

A

protons and electrons

39
Q

This property results in a cation

A

ionization energy

40
Q

The energy required to remove an electron from a neutral atom

A

ionization energy

41
Q

This property increases down a group and decreases across a period

A

atomic radius (atomic size)

42
Q

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

A

electronegativity

43
Q

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

A

Seaborg

44
Q

He grouped elements into triads

A

Dobereiner

45
Q

He proposed the law of octaves

A

Newlands

46
Q

He arranged the periodic table according to increasing atomic number

A

Moseley

47
Q

Both of these scientists arranged elements according to increasing atomic mass

A

Mendeleev and Meyer

48
Q

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

A

transition elements

49
Q

These elements rarely form compounds

A

noble gases

50
Q

This group loses two electrons

A

akkalune earth metals

51
Q

These are the most reactive of the nonmetals

A

halogens

52
Q

Which element has more metallic character

A

Sulfur

53
Q

Which element is smaller

A

Fluorine

54
Q

Which element has a lower electronegativity

A

Sodium

55
Q

Which element has a larger radius

A

Francium

56
Q

Which element has a stronger electron affinity

A

Carbon

57
Q

Which metal is the most reactive

A

Potassium

58
Q

Which nonmetal is the most reactive

A

Fluorine

59
Q

Explain why smaller atoms have greater ionization energies

A

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

60
Q

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?

A

It can strongly attract a shared pair of electrons toward itself

Chem Honors (6 decks)

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