CHEM126 – ACS I

 

ACS I

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Question 1

 

How many atoms are in 1.75 g of Na?

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Question 2

 

The element X occurs naturally to the extent of 65.52% 30X and the rest 32X. What is the atomic mass of X? (Use 4 sig. fig.)
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Question 3

 

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Question 4

 

What is the expected empirical formula of gallium oxide?
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Question 5

 

Which ion does not have 18 electrons?
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Question 6

 

What is the maximum number of electrons that can occupy a px orbital?
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Question 7

 

What is the valence electron configuration of the element in Period 4, Group 4A?
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Question 8

 

Four of the five d orbitals could be represented by
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Question 9

 

What is the electron configuration of Mn5+ in the ground state?
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Question 10

 

Which electron configuration is impossible? (Careful, excited states are possible.)
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Question 11

 

How many unpaired electrons does Co2+ have?
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Question 12

 

which of these species is paramagnetic?
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Question 13

Which of these diagrams could represent the ground state of the d valence electrons of V?

 

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Question 14

 

Which set of quantum numbers is correct and consistent with n = 3? (l = angular momentum quantum number, ml = magnetic q.n., and ms = electron spin q.n.)
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Question 15

How many sigma bonds and pi bonds are in this structure?

 

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Question 16

 

Arrange the nitrogen-nitrogen bond lengths in order from shortest to longest for N2, N2H2, N2H4.
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Question 17

 

An ionic substance typically exhibits all of the following properties except
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Question 18

The Lewis structure for Sulfur dioxide can be described by two resonance structures: 

 

These resonance structures indicates that the

 

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Question 19

 

Which concept(s) explain why the water molecule is bent and that the angle is about 105º?
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Question 20

 

Which statement is incorrect about the boiling points for the 6A hydrides: H2O, H2S, H2Se, and H2Te
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Question 21

 

Which of the following molecules is nonpolar?
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Question 22

 

The molecule of the type ML4E2 consists of four single bonds and two lone pairs. What structure is it expected to assume?
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Question 23

 

In which pair are the molecules geometrically similar?
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Question 24

 

Which molecule is planar?
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Question 25

 

What set of species is arranged in order of increasing S-N-S bond angle?
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Explanation

Remember lone pairs of electrons are bulkier than bonding pairs.

Question 26

 

What type of hybrid orbital is used in PCl5?
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Question 27

The molecule OCNH (shown below) has been detected in gas clouds between stars. The predicted O-C-N bond angle is about

 

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Question 28

 

MA2B2 is a molecule where M is the central atom bonded to 2 atoms of A and 2 atoms of B. The fact that it exists in only one form (no isomers) suggests its geometry is
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Question 29

 

A compound is found to consist of 28.1% sodium, 13.2% boron and 58.7% oxygen. What is its simplest formula?
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Question 30

 

A compound is found to consist of 28.1% sodium, 13.2% boron and 58.7% oxygen. What is its simplest formula?
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Question 31

 

A 4.000 g sample of an unknown metal, M, was completely burned in excess O2 to yield 0.02225 mol of the metal oxide, M2O3. What is the metal?
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Question 32

 

What is the maximum mass in grams of aluminum chloride that could be obtained from 2.50 mol of barium chloride and excess aluminum sulfate? This is the balanced equation for the reaction: Al2(SO4)3 + 3BaCl2–> 3BaSO4 + 2AlCl3. BaCl2 molar mass is 208.3 g/mol and AlCl3molar mass is 133.3 g/mol.
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Question 33

 

1.0 x 10-5 g sample of a compound is known to contain 1.36 x 1017 molecules. This compound is
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Question 34

 

1.438 g sample of a compound of nitrogen and oxygen contains 1.000 g of oxygen. What is the empirical formula?
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Question 35

 

The limiting reagent in a particular reaction can be recognized because it is the reagent that
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Question 36

Consider this reaction used for the production of lead. What is the maximum mass of lead that can be obtained by the reaction of 58.0 g PbO and 30.0 g ofPbS?

 

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Question 37

What volume of 0.20 M BaCl2 is required to react completely with 25.0 mL of 0.600 M Na2SO4? This is the net ionic equation for the reaction:

 

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Question 38

 

What is the molarity of a solution made by dissolving 3.95 g of sodium acetate in water and diluting to 750. mL? (molar mass NaC2H3O2 is 82.0 g/mol.)
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Question 39

An open-ended mercury manometer is used to measure the pressure exerted by a trapped gas as shown in the figure. Atmospheric pressure is 750. mmHg. What is the pressure (in mmHg or torr) of the trapped gas if h =28 cm?

 

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Question 40

 

What volume (in mL) of 12 M HCI solution is required to prepare exactly 500. mL of a 0.55 M HCI solution?
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Question 41

 

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Question 42

 

A particular solid is soft, a poor conductor of heat and electricity, and has a low melting point. Generally, such a solid is classified as
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Question 43

 

The boiling point of an impure compound is generally
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Question 44

Given the cooling curve of one gram of a pure liquid, the length of the line BC depends on

 

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Question 45

Which phase has the largest specific heat? (Hint, how are the slope and specific heat related?)

 

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Question 46

 

What is the molar mass of an ideal gas if a 0.800 g sample of this gas occupies a volume of 200. mL at 50.0 oC and 720. mm Hg?
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Question 47

 

What is the molar mass of an ideal gas if a 0.800 g sample of this gas occupies a volume of 200. mL at 50.0 oC and 720. mm Hg?
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Question 48

 

Copper crystallizes in a face-centered cubic lattice. What is the mass of one unit cell? Report your answer in grams.
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Question 49

 

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Question 50

 

When a 90 g sample of an alloy at 100.0 oC is dropped into 90.0 g of water at 24.6 oC, the final temperature is 34.1 oC. What is the specific heat of the alloy? (The specific heat of water is 4.184 J/(goC).)
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Question 51

 

What is the enthalpy of formation of CO(g) in kJ? 2CO(g) + O2(g) –> 2CO2(g). ΔH reaction = -566 kJ ; ΔH CO2(g) =-393.5 kJ/mol.
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Question 52

 

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Question 53

When 137 J of energy are added to a sample of gallium that is initially at 25.0 oC, the temperature rises to 48.0 oC. What is the volume of the sample in cubic centimeter?

 

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Question 54

Calculate the change in enthalpy for the chemical reaction N2(g) + 3H2(g) –> 2NH3(g)

 

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Question 55

The following question is from the ACS Study Guide. It would be better to ask which diagram best represents the change in enthalpy for the dissolution process.

 

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Question 56

 

For which of the following reaction is the enthalpy of formation of the compound equal to the ΔH of reaction?
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Question 57

Which of these elements is predicted to be the most active nonmetal?

 

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Question 58

 

When C30H50O2 is completely oxidized with excess oxygen, what are the products?
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Question 59

 

In what part of the periodic table are the largest electronegativities found?
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Question 60

 

Which gas is LEAST soluble in water?
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Question 61

 

In what part of the periodic table are the smallest ionization energies for the first electron found?
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Question 62

 

Arrange the elements Li, Be, Ne, and Ar in increasing order of the energy required to remove an electron from their respective gaseous atoms.
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Question 63

 

The first four ionization energies of an element X are 0.58, 1.82, 2.74, and 11.58 MJ/mol. What is the most likely formula for a stable ion of X?
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Question 64

 

If the formula of an oxide of element X is XO, what is the formula of the nitride of X?
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Question 65

 

When the three ions N3-, O2-, and F- are arranged in order of increasing ionic radius, which is the correct order?
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Question 66

 

When the three elements P, Cl, and As are arranged in order of increasing atomic radius, which is the correct order?
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Question 67

 

In what part of the periodic table are the largest atoms found?
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Question 68

 

Which is a characteristic property of transition elements?
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