Free Printable chemistry final

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chemistry final

Total questions: 148

Worksheet time: 2hrs 28mins

Name

Class

Date

how would you classify an element with the electron configuration?

Kr, 4d8 5s2

a transition metal

an alkali metal

an alkali earth metal

a halogen

the symbol and atomic mass of the halogen in period 4 are what and what?

Cl, 35.453 (atomic mass)

Br, 79.90 (atomic mass)

F, 18.99 (atomic mass)

the symbol and number of protons of the period 3 alkali metal are what and what?

Mg, 12 protons

Na, 11 protons

Be, 4 protons

concentrated sulfuric acid is 95% sulfuric acid by mass, and has a density of 1.84 g/ml. what is the volume of concentrated sulfuric acid solution that has 14. 9 g of sulfuric acid?

8.52 ml

5.56 ml

7.69 ml

9.26 ml

The combustion of butane (C₄H₁₀) produces CO₂ and H₂O. When 0.335 mol butane is burned in excess oxygen, how many moles of carbon dioxide are formed?

1.36

1.34

1.38

$N_2^{ }\left(g\right)+3H_2^{ }\left(g\right)-\ 2NH_3\left(g\right)$

How many grams of NH3 can be produced by the reaction of N2 with 3.00 g H2?

0.964 g

2.43 g

4.00

17.0

$2NaN_3-2Na+3N_2$
if you start with 47.5 g NaN3 and produce 30.0 g of N2, the percent yield of N2?

92.7 %

67.5%

56.2%

97.7 %

$2Mg\left(s\right)+O_2\left(g\right)-2MgO\left(s\right)$
when 10.1g of Mg with 10.5 g of O2, 11.9g of MgO are produced (actual yield). determine the limiting reactant and the percent yield?

Lr = 16.75 g / 71.0 %

Lr= 15.65 g? 61 %

$4NH_3\left(g\right)+5O_2\left(g\right)-4NO\left(g\right)+6H_2O$
how many mole of NH3 are required to completely react with 14.5g O2?

12.2 mole

11.6 mole

13.5 mole

10.

$4NH_3+5O_2-4NO+6H_20$
how many grams of NO are formed by the complete reaction of 14.5 g O2?

10.9g

11.1 g

10.5 g

11.

what does ite, and ate represent?

ite- NO2 smallest

ate- NO3 Plus largest

ite - NO3 smallest

ate- NO2 largest

12.

what is the strong electrolyte?

a substance that completely dissociates into ions when dissolved in water.

a substance that does not dissolve in water.

13.

$HNO_3\left(aq\right)+NaOH-\ NaNO_3\left(aq\right)+H_2O$

which is the correct net ionic equation?

$H^{-\ }\left(aq\right)+OH^+\left(aq\right)-H_2O\left(l\right)$

$H^+\left(aq\right)+OH^-\left(aq\right)-H_2O\left(l\right)$

14.

$Pb\left(NO_3\right)_2^{ }\left(aq\right)+2LiCl\left(aq\right)-PbCl_2\left(s\right)+2LiNo_3\left(aq\right)$ which of the following is the correct net ionic eqaution?

$Pb^2\left(aq\right)+2cl\left(aq\right)-PbCl_2\left(s\right)$

$Pb^4\left(aq\right)+3cl^-\left(aq\right)-PbCl^2\left(s\right)$

15.

choose the true statement?

The actual yield is the amount of product actually produced by a chemical reaction

The percent yield = Actual Yield/Theoretical yeld × 100%

The limiting reagent determines the theoretical yield of the product

The limiting reactant is completely consumed in a chemical reaction

The actual yields must be determined experimentally

16.

Which of the following reactions results in the following net ionic equation:

H⁺(aq) + OH^-(aq) → H₂O(l)

4 NH₃(g) + 5 O₂(g) → 6 H₂O(g) + 4 NO(g

HCl(aq) + KOH(aq) → H₂O(l) + KCl(aq)

2 H₂(g) + O₂(g) → 2 H₂O(g

HClO₄(aq) + LiOH(aq) → H₂O(l) + LiClO₄(aq)

17.

When aqueous solutions of lead (II) nitrate and potassium iodide are mixed, a precipitate forms. What is the net ionic equation for this process?

Pb²⁺(aq) + 2I-(aq) → PbI₂(s

Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂ (s) + 2K⁺(aq) + 2NO₃^-(aq

Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(aq

K⁺(aq) + NO₃^-(aq) → KNO₃(s

18.

What mass of chlorine gas, in grams, is needed to react completely with 16.3 g of aluminum?

2Al(s)) + 3Cl₂(g) → 2AlCl₃(s)

61.26

63.20

64.24

19.

Consider the reaction: 4Al(s) + 3O₂(g) → 2Al₂O₃(s)

What is the percent yield of aluminum oxide when 122 g Al react with excess oxygen to produce 185 g of aluminum oxide?

80.3

79.1

80.2

20.

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below

N₂(g) + 3 H₂(g) → 2 NH₃(g

3.3 g of hydrogen are left over

Hydrogen is the excess reactant

Nitrogen is the limiting reactant

The theoretical yield of ammonia is 15 g.

21.

Consider the following reaction: 4 Al + 3 O₂ → 2 Al₂O₃

A mixture of 82.5 g of aluminum and 117 g of oxygen is allowed to react. What mass of aluminum oxide can be formed?

152

150

156

22.

Consider the reaction: 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g).

If the reaction of 150. 0 g of ammonia (NH₃) with 150.0 g of oxygen gas produce 87 g of nitrogen monoxide (actual), then what is the percent yield of this reaction?

76.2

77.3

77.4

23.

Consider the reaction: 3 Mg + N₂ → Mg₃N₂

A given reaction yielded only 6.0 g of the Mg3N2 which represents a 50 % yield. How many grams of N2 reacted?

3.3

3.2

3.5

24.

$2Al+\ 3Cl_2-2AlCl_3$

Many metals react with halogen to give metal halides,

you will need 23.6 Clsquare for complete reaction and will produce 66.7g of AlCl

you will need 53.3g Cl for a complete reaction and will produce 66.7 g of AlCl.

you will need 26.6g Cl for complete reaction and will produce 49.0g of AlCl

25.

$4Al\left(s\right)+3O_2\left(g\right)-2Al_2O_3\left(s\right)$
how many grams of Al are needed are produce 112 g of Al2O3 (actual) if the reaction has 80.5%yeied .

73.7g

81.3 g

75.2

9.1

26.

aluminum metals reacts with iron (iii) to form aluminum oxide and iron metal. what is the stochemetric coefficient for aluminium when the chemical equation is balanced using the lowest, whole number stoichemetric coefficients?

27.

how many hydrogen atoms are thre in 1.0 micrograms of water?

1.2 x 10^18 atoms H

1.1 x 10^22 atoms H

6.7 x 10^16 atoms H

28.

what mass of Al(NO3)3 will contain 5.00 x10^24 oxygen atoms?

196g

98.4

23.7

590 g

29.

a sample of NaClO3 contains 6.00g Na. find the mass of oxygen in the same sample?

8.62g

2.88

12.5g

9.26

30.

Rank the following bonds in order of increasing polarity.

I. F-O II. F-C III. F-N IV. F-F

IV, I, III, II

II, III, II, IV

I, II, III, IV

31.

Whichof the following species is polar? Choose all that apply.

SO₂

CO₂

CCl₄

NCl₃

32.

Which of the following compound is correctly name? Choose all that apply?

FeCl₃ Iron(III) chloride

Mg₃N₂ magnesium nitride

AlCl₃ aluminum trichloride

Na₂SO₄ sodium sulfate

N₂O₅ dinitrogen pentoxide

33.

The formulae of the sulfate ion, the ammonium ion and the chlorate ion are represented by, respectively as:

S^2-, NH₄⁺, ClO₂

SO₄^2-, NH₄⁺, ClO₃^-

SO₃^2-, NH₂^-, ClO₃^-

S^2-, NH₂⁺, ClO₂^-

34.

Calculate the number of oxygen molecules required to produce 16.1 g KHCO₃.

1.45*10^23

1.22 *10^23

1.30*10^21

35.

Choose the true statements. Choose all that apply.

One mole of H₂O contains the same number of molecules as one mole of H₂

One mole of H₂O contains one atom of O

One mol of H₂O contains two mol of H

The mole is a SI unit for counting atoms, molecules, or ions

36.

Calculate the molar mass of calcium phosphate. Express your answer in decimal with 4 significant figures. Do not include the units

310.1

220.5

120.6

120.8

37.

A sample of dinitrogen trioxide contains 4.53 x 1022 molecules. What is its mass?

7.86

3.35

5.72

38.

Determine the volume of hexane that contains 5.33 × 10²² molecules of hexane. The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.

10.5

11.6

9.8

39.

Calculate the mass % of oxygen in aluminum sulfate. Provide answer to 3 significant figures

56.1

20.2

18.9

40.

what is the molecular of NOCl as predicted by the VSEPR theory?

linear

trigonal planer

bent

tetrahedral

41.

a compound 49.32% C, 43.83%, and 6.85%H, what is the empiral formula?

$C_3HO_3$

$C_3H_3O_4$

$C_2HO_3$

$C_3H_5O_2$

42.

$ClO^-,\ IO_3\ ,\ NO_2$

what is the correct set of names for the annions listed?

chorite, periodate, nitrate

hypochlorite, iodite, nitrtate

perchlorate, periodate, pernitrate

hypochlorite, iodate, nitraite

43.

how many lone pairs of electrons are there in the lewis structure of NOCl (N is the central atom)?

44.

A general chemistry students was asked to name to the following compounds, the students answers are given below?

HBrO4

AlPO4

HNO2

Al2O3

FeCl4

45.

when calcium reacts with bromine it forms?

an ionic compound CaBr

an ionic compund CaBr4

46.

order the elements in S, Cl, and F increasing atomic radius (smallest to highest )

S, Cl, F

Cl, F, S

F, S, Cl

F, Cl, Sb

47.

choose all that appy?

An ionic bond is the transfer of electrons from one atom to another

A covalent bond is the sharing of electrons between atoms

The chemical formula for the compound formed between Al and O is AlO

The Lewis symbol for O has 2 unpaired electrons

48.

Determine the charge of the unknown ion, X, in each of the following compounds:

(a) X₂O (b) SrX (c) K₃X (d) X₂O₃

-2

-3

49.

Which combination of elements would be most likely to form covalent bonds?

choose that all apply

Nitrogen-oxygen

carbon-sodium

carbon-fluorine

cesium-fluorine

50.

Potassium metal and chlorine react vigorously to form potassium chloride.

Each K atom loses an electron and becomes an Ar atom

Each Cl atom gains an electron and becomes an Ar atom

Each Cl atom gains an electron and attains the electron configuration of an Ar atom

51.

The total number of lone pairs of electrons in the following molecules/ions are:

NCl_{3 - 10}

SeO₂ - 6

CO₂ - 4

[NH₄]⁺

= 0

52.

Which one of the following species contains a triple bond?

NO₃^-

CO₂

CN^-

HCN

53.

What is the approximate bond angle in the following molecules/ions are:

NCl₃ = 109

SeO_{2 = 120}

CO₂ = 180

: [NH₄] = 109

54.

What is the correct formula of a compound between calcium and nitrogen?

Ca- Ca3

Ca- Ca2

N- N2

N- N3

55.

What is the electron group geometry around the central atom in the following molecules/ions ?

i SeO₂

tetrahedraal

trigonal planar

bent

56.

What is the electron group geometry around the central atom in the following molecules/ions ?

i ClO₃^-

Tetrahedral

trigonal plannar

linear

tetrahedral

57.

What is the electron group geometry around the central atom in the following molecules/ions ?

i CO₂

trigonal planar

tetrahedral

linear

bent

58.

What is the electron group geometry around the central atom in the following molecules/ions ?

i NH₃

Tetrahedral

bent

linear

59.

What shapes do the following molecules/ions have?

i SeO₂

bent

trigonal pyramidal

linear

60.

what is the best shape that decribes this molecule?

ClO₃^-

linear

bent

trigonal pyramidal

61.

What shapes do the following molecules/ions have?

ClO₂^-

bent

trigonal pyramidal

linear

62.

What shapes do the following molecules/ions have?

HCN?

trigonal pyramidal

linear

bent

63.

what is the best shape that decribes this molecule?

ClO₃^-

linear

bent

trigonal pyramidal

64.

describes the electron geometry and molecular geometry for NF3 and H2O?

NF3= tetrhedral, triginal pyramid

NF3= trtrahedral, vent

H2O= tetrahedral, bent

H2O= trigonal planar, bent

65.

which of the following statement is correct?

SeO2 = bent, nonpolar

AlCl= tetrahedra, polar

CO2 = linear, nonpolar

H2O = bent, nonpolar

66.

how many protons, neutrons, and electrons, are there in the most likely cation formed from barium 140?

56, 84, 54

84, 56, 56

54, 84, 56

67.

an atom of flourine contaims 9 electrons. how many electrons are in P orbitals

68.

$32s^2,\ 40Ar,\ \ 39\ K\$

what do the following three species have in common?

The number of protons

the number of neutrons

the number of electrons

the mass number

69.

which of the folloeeing elements would have 3 singly occupied orbitals in it's ground state.

X cobalt

Y aluminuim

z Arsenic

X only

y only

Z only

X and Z only

70.

which of the folloeeing is not capable of having resonance structures?

SeO2

NO3

SO2

H2O

71.

all of the following have the same general shape as H2O except?

NH2

CCl2

CO2

72.

consider the two compounds, NOF and NO2F which of the following statement is true? N is the central atom?

NOF Is linear, NO2F is planar

NOF is bent, NO2F is planar

NOF is planar, NO2F is bent

73.

$32s^2,\ 40Ar,\ \ 39\ K\$

what do the following three species have in common?

The number of protons

the number of neutrons

the number of electrons

the mass number

74.

put the following atoms in order of increasing first ionization energy, Cs, He, C, O, Sr

Cs, Sr, C, O, He

Cs, Sr, O, C, He

He, O, C, Sr, Cs,

75.

All of the ---- have a valence shell electrons configurations ns2, np5?

noble gas

halogens

alkaline metals

alkaline earth metals

76.

give the ground state electron configuration for Mg2 plus?

1s2, 2s2, 2p6, 3s2

1s2, 2s2, 2p6,

1s2, 2s2, 2p6, 3s2, 3p2

77.

chlorine has two stable isotopes, 35l and 37 Cl, =. if their exact masses are 24.9689 amu and 36.9695 amu and the narural abundance of 35 Cl (the atomicc mass of chlorine is 35.345 amu)

75.95%

24.05%

50.00 %

78.

which of the following are true statement ?

X the mass of 1 of carbon 12 is exactly 12

Y carbon contains at least one natural istope heavier than carbon

z the mass of one atom of carbon 12 is 1.99 x 10^23

X only

Y only

Z only

X, Y, Z

79.

which one of the following atoms would you expect to lose electrons when forming ions?

X Al

Y Na

Z Te

W p

Y and Z

Y only

X only

X and Y

80.

whic of the following statements about physical and chemical chnage is false.

in a chemical change, matter chnages it's composition

in a physical chnage, matter does not change it's composition

Phase changes are always physical changes

All of the above statements are true

81.

which of these molecules is nonpopar?

H2O

NF3

SO3

HCl

82.

which of the following is false?

matter may be a pure substance or it may be a misture

a pure substance may either be an element or a compound

a mixture may be either homogenous heterogenous

mixture may be composed of two or more elements, two or more compounds, or combination of both.

all of the about statements are true

83.

the average density of the earth is 6.52g/ cm cube. what volume in meter cube will 4.5x 10^4 microgram occupy?

1.9 x10^ -6

4.6 x 10 ^-7

6.1 x 10^ 6

6.9 x 10^ -9

84.

a homogenous mixture was prepared by mising 0.15g A, 112.3g B and the 24.55g C. the volume is found to be 85.60 cm cube. what is the density of the misture to correct number of significant digifits?

1.5967 g

1.59674 g

1.6 g

1.597 g

85.

The Si prefixes gigi and nano represent respectively?

10^6 and 10^ -6

10 ^9 and 10 ^ -6

10^9 and 10 ^ -9

86.

newton is the Si unit of force (mass x acceleration) hoe is newton defined in terms of base SI units ?

Kg - m.s

kg. m square. s square

Kg . m. s square

87.

the density of silver is 10.5 g/ cm cube. how many Ag atoms are present in a silver bar that measures 0.1000m x 0.05000m x 0.0100m?

2.93 x 10^ 24 atoms

5.63 x 10^ 23 atoms

1.93 x 10^22 atoms

88.

The width, length, and height of a large, custom-made shipping crate are 1.22 m, 3.22 m, and 0.54 m, respectively. The volume of the box using the correct number of significant figures:

2.12134 m³

2.1 m³

2.12 m³

89.

The mass of a proton is 1.67 × 10^-27 kg. What is the mass of a proton in milligrams?

1.67 × 10^-27 mg

1.67 × 10^-24 mg

1.67 × 10^-21 mg

90.

The mass of a proton is 1.67 × 10^-27 kg. What is the mass of a proton in milligrams?

1.67 × 10^-27 mg

1.67 × 10^-24 mg

1.67 × 10^-21 mg

91.

If the density of an object is 80.06 lb/ft³, then the density in g/cm³ is:

(1lb = 454 g, 1 in=2.54 cm, 1 ft = 12 in)

1.29 g/cm³

3.92 g/cm³

0.88 g/cm³

92.

The average density of the earth is 6.52 g/cm³. What volume in m³ will 2. 0 x 10⁴ µg occupy?

4.6 x 10^-7 m³

6.1 x 10^-6 m³

3.1 x 10^-9 m³

93.

When combining the masses 0.1569 kg, 2.43 mg and 20.476 g. The total mass should be reported as:

177.378 g

177.4 g

177.37 g

177.38 g

94.

Calculate the speed, in m/s, of a car traveling 80.0 miles per hour. (1 mile = 1.609 km)

45.6 m/s

25.2 m.s

35.8 m/s

95.

The density of an object is 2.7 g/cm³. What is its density in kg/m³?

2.7 x 10⁴ kg/m³

2.7 x 10³ kg/m³

2.7 x 10^-3 kg/m³

96.

The density of lead is 708 lb/ft³. What is this density expressed in SI base units?

(1 lb = 454 g, 1 in = 2.54 cm, 1 ft = 12 in)

2.14 x 10^-2 kg/L

1.14 x 10⁴ kg/m³

3.14 x 10⁷ g/m³

97.

Pressure is defined as force/area and force equals mass times acceleration. The S. I. unit of pressure is the Pascal and the basic SI units for a Pascal are:

kg m^-1 s^-3

kg m^-1 s^-2

kg m^-2 s^-2

98.

A slab of patio brick (d = 3.4 g/cm³) is cut into a perfect square 5.35 cm on a side and has a mass of 0.47 kg. What is the thickness of the brick?

5.6 cm

2.8 cm

6.6 cm

4.8 cm

99.

Choose the true statements. Choose all that apply

A compound can be decomposed by simple chemical changes

Surface area and volume are both extensive properties

Density and boiling point are physical properties

Density and boiling point are both intensive properties

A mixture is always a homogeneous combination of different substances

100.

The symbol and atomic number of the halogen in Period 5 is

I, atomic number 53

Ba, 137

101.

By knowing the number of protons in a neutral element and looking at the periodic table, we also know:

the number of electrons in the element

the symbol of the element

the number of neutrons in the element

the mass number of the element

102.

Each of the following orbital pictures are in the energy level n = 3, label them with the appropriate number and letter.

3p, 3s, 3d

3s, 3p, 3d

103.

Identify the element represented by each of the following ground-state electron configurations:

X = [Ar] 4s²3d⁷ Y = [Ar] 4s²3d¹⁰4p⁵ Z = 1s²2s²2p⁶3s²3p¹

X = CO

Y= Br

Z= Al

104.

How many unpaired electrons are in the ground state electron configurations of S, As, Ne?

S= 4

AS = 3

Ne= 0

none of the above

105.

Consider the following species: ⁴¹Ca²⁺ and ³¹P^3--

They are ions

They have the same number of neutrons

They have the same number of electrons

They have noble gas configurations

106.

A 2.5-carat diamond cost $8500. What is the price of one carbon atom in this diamond? (Diamond is 100% carbon; 1 carat = 200 mg; N_A = 6.023 x 10²³ mol^-1)

8.34 x 10^-25

5.22 x 10^-24

3.38 x 10^-19

107.

Choose the true statements. Choose all that apply

A charged atom (ion) must contain more electrons than protons

The mass of electrons in an atom does not have considerable effect on the mass of that atom

A different element is formed by changing the number of protons in an atom’s nucleus

The mass number of an element equals the number of protons plus the number of neutrons.

108.

A 125 mg sample of an element contains 1.34 6x 10²¹ atoms. What is this element? (N_A = 6.023 x 10²³mol^-1)

109.

An aqueous solution has a density of 1.13 g/mL and contains 6.00% sugar by mass. What volume of this solution contain 255 grams sugar?

2.55 x 10³ mL

1.22 x 10³ mL

3.76 x 10³ mL

110.

What is the volume of a block of iron containing 3.97 x 10²⁴ atoms? Density of iron: 7.87 g/cm³(N_A = 6.022 x 10²³ mol^-1)

46.8

30.2

22.6

111.

Place the following in order of increasing atomic radius: S Na Li

smalles to largesr

Li, S, Na

Na, Li, S

S, Na, Li

112.

Place the following in order of increasing ionization energy: Cl Mg Ba

lowest to highest

Mg, Cl, Ba

Cl, Mg, Ba

Ba, Mg, Cl

113.

choose the smaller species?

i P or P3-

ii Al or Al3+

P3-

Al3+

114.

Which of the following are physical changes?

W the evaporation of water

X burning of wood

Y Dissolution of sugar

W and Y

X and Y

Y and Z

W and X

115.

An aqueous solution has a density of 1.13 g/mL and contains 12.0% sugar by mass. What volume of this solution contain 255 grams sugar?

2.55 x 10^3 ml

2.34 x 10^3 ml

1.88 x 10^3 ml

116.

choose the correct statements?

The principal quantum number (n) determine the energy of an orbital

Part of the Bohr model proposed that electron in the hydrogen atom is located in "stationary states" or particular orbits around the nucleus

The number of orbitals in a given subshell is 7

An orbital is the volume in which we are most likely to find an electron

117.

by knowing the number of protons in a neutral atom we alo know?

X number of electrons in the atom

Y the sybol of the element

z the number of neutrons in the atom

X and Y only

X and Z

118.

which of the following about subatomic particles is true?

protons have about the same mass as electrons

electrons make up most of the mass of an atom

a neutral atom contains the same number of protons and electrons.

119.

how many atoms of oxygen are in 25 mg aluminum sulfate?

6.022x 10^23 mol

5.28x 10^20 atoms

4.88 x 10^21 atoms

2.22 x 10^15 atoms

120.

what is the difference betwee mass number and atomic number?

mass number, number of protons and neutrons.

atomic number, number of weighted average of isotropes.

mass number; average density of mass

atomic number; number of protons and electrons

121.

sodium chloride can be produced by evaporating seawater to dryness. what volume of seawater in liters must be evaporated to dryness to produce 751 g sodium chloride? the density of seawater is 1.03 g/ ml and seawater is 3.5 % sodium chloride by mass?

20.8 L

19.2 L

35.6

122.

what is the definition of cation and anion?

anion; loses electron

cation; gains electron

anion; gains electron

cation ; loses electron

123.

what is the definition of isotope and atomic mass?

istope; charging electrons

atomic mass; the number of protons and neutrons

atomic mass; the weighted average of all occuring istope.

isotope; the numbers of neutrons charge.

124.

what is the definition of element anf compound?

element; is any substance that can be broken down

compound is composed of two or more elements

compound; is a substance that can be broken down

element; is composed of two or more elements

125.

A 75g of sodium chlordie is to be produced by evaporatin to dryness a quantity of sea water containing 3.5% sodium chloride by mass. what volume of seawaetr in liters must be taken for this purpose?

assume the density of 1.03g/ml for seawater.

3.2 L

2.1 L

5.2 L

126.

An intravenous bag delivers a nutrient solution to a hospital patient at a rate of 1.5 drops per minute, A drops weigh 65 mg on average. how many kilograms of solution are delivered in 4.0h?

2.3 *10^-3 kg

1.5 *10^-2 kg

4.6*10^-5 kg

127.

Choose the true statements. Choose all that apply

Two electrons in the same orbital must have opposite spin

An orbital is the path that an electron follows during its movement around the nucleus

One mole of chlorine has a mass of 35.45 amu

The mass of 1 mol of carbon-12 is exactly 12 g

128.

choose the correct statements?

The principal quantum number (n) determine the energy of an orbital

Part of the Bohr model proposed that electron in the hydrogen atom is located in "stationary states" or particular orbits around the nucleus

The number of orbitals in a given subshell is 7

An orbital is the volume in which we are most likely to find an electron

129.

An element consists of two isotopes of masses 68.95 amu and 70.95 amu. The relative abundance of the first one is 60.16 %. What is the average atomic mass of the element based on this data? (Express your answer in decimal notation with 4 significant figures and do not include the unit)

69.75

50.60

20.65

130.

The average atomic mass of copper is 63.5 amu. Copper has two naturally occurring isotopes. One of the isotopes has atomic mass of 62.9 amu and an abundance of 69.1 %. Calculate the atomic mass (amu) of the other isotope.

64.8

60.5

60.6

131.

An element has three naturaly occuring isotopes with the mass and natural abundances given here. Calculate the atomic mass of the element

19.06

28.08

25.07

132.

Copper has a density of 8.96 g/cm³. How many kg of copper occupy 5.00 m³?

4.48 *10^4

2.27*108

3.35*10^9

133.

Copper has a density of 8.96 g/cm³. How many m³ of copper weight 3.40 kg? ?

5.69*10^-2

3.79*10^-4

22.8*10^-6

134.

An element has three naturaly occuring isotopes with the mass and natural abundances given here. Calculate the atomic mass of the element

19.06

28.08

25.07

135.

place the following in order of increasing atomic radius

smallest to largest

I As

ii O

iii Br

O, Br, As,

As, Br, O

Br, O, As

136.

place the following in order of increasing ionization?

lowest to highest

i K

ii Ca

III Rb

Ca, Rb, K

Rb, K, Ca

K, Ca, Rb

137.

concentrated sulfuric acid is 95% sulfuric acid by mass, and has a density of 1.84 g/ml. what is the volume of concentrated sulfuric acid solution that has 14. 9 g of sulfuric acid?

8.52 ml

5.56 ml

7.69 ml

9.26 ml

138.

order the four metric units from smallest to largest?

i kilometer

ii nanometer

iii millimeter

iv micrometer

2, 4,3, 1

1,2, 3, 4

4, 2, 3, 1

139.

What is the symbol of element Q if the ion Q²⁺ contains 18 electrons?

140.

What is the volume of a block of iron-containing 7.93 x 10²⁴ atoms? The density of iron: 7.874 g/cm³

93.4

50.6

44.8

141.

A sample of Ne consists of the following:

Isotope (amu) % abundance

²⁰Ne(20.04 amu) 66.80%

²¹Ne(20.97 amu) 1.40%

²²Ne(21.83 amu) 31.80%

What is the molar mass of the Ne sample?

20.41 g/mol

19.50 g/mol

20.62 g/mol

142.

A certain element has just one natural isotope. If 6.4 ng of this element contains 3.04 x 10¹³ atoms, identify the element.

(N_A = 6.022 x 10²³ mol^-1

Beryllium

Iodine

Gallium

143.

Calculate the mass (in kg) of 4.87×10²⁵atoms of Zn. (molar mass of Zn = 65.39 g/mol; N_A = 6.022 x 10²³ mol^-1)

8.09 kg

5.29 kg

1.24 kg

144.

How would you classify an element with the following electronic configuration [Kr]5s²?

a transition metal

an alkaline earth metal

a halogen

145.

choose the bigger species

i Br or Br-

ii Ca 0r Ca2+

iii K or Br

iv Mg or Ba

Br-

146.

What is the symbol of element Q if the ion Q³⁺ contains 10 electrons?

147.

How many unpaired electrons are in the ground-state electron configuration of C, S, and N?

C= 2

S= 2

N= 3

148.

Which of the following have unpaired electrons?

I. Ni II. C III. S^2- IV. Mg²⁺

I, II, III and IV

I and II

III and IV

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chemistry final

Total questions: 148

Worksheet time: 2hrs 28mins

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