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Chemistry > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

Sulfur mustard or mustard gas is a chemical weapon that causes blisters on the skin and in the lungs. Its chemical formula is C4H8Cl2S. What is the molar mass of this compound?

A

M = (4 x 12.01g/mol) + (8 x 1.008g/mol) + (2 x 35.45g/mol) + (1 x 32.07g/mol) = 159.074g/mol

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2
Q

The smallest particle of an element that retains the chemical properties of that element.

A

Atom

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2
Q

A model of the atom that assumed the electrons were negatively charged particles spread throughout a diffuse, positively charged matrix.

A

The Plum Pudding Model

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2
Q

The short range proton-neutron, proton-proton, and neutron-neutron forces that hold the nuclear particles together

A

Nuclear Forces (or the Strong Force)

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2
Q

Strontium nitrate is used as a red colorant in fireworks. The formula for the compound is Sr(NO3)2. What is the formula mass of this compound?

A

M = (1 x 87.62u) + (2 x 14.01u) + (6 x 16.00u) = 211.64u

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2
Q

How many formula units are there in 0.084mol of potassium sulfide, K2S?

A
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2
Q

How did Rutherford explain the mass and volume of the nucleus?

A

The nucleus occupies only a tiny volume of the entire atom, yet contains over 99.9% of the atom’s mass. Therefore it is a very dense, positively charged area.

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3
Q

The tiny central core of an atom having a dense, positive charge

A

Nucleus

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5
Q

A symbol that indicates the identity of a particular atom using its symbol, along with the number of protons as a subscript and the mass number as a superscript, preceding the symbol.

A

Nuclide symbol

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5
Q

A mass defined as being exactly 1/12th the mass of a carbon-12 atom.

A

Atomic mass unit (u or amu)

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6
Q

The identity of an atom is determined by the number of these in the atom.

A

Protons

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7
Q

The total number of protons and neutrons in a nucleus

A

The mass number (A)

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8
Q

What is the mass of 0.085mol of iodoform (CHI3), a chemical used as a disinfectant, whose smell is sometimes described as the smell of a hospital?

A
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9
Q

A neutral subatomic particle, found in the nucleus of an atom.

A

Neutron

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10
Q

The general term for a specific isotope of an element

A

Nuclide

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12
Q

Calculate the number of moles of lithium sulfate in a 16.5g sample of the compound.

A
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14
Q

A law that states that “a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound.”

A

The Law of Definite Proportions

15
Q

How many moles are there in a 2.61g sample of aluminum carbonate, Al2(CO3)3?

A
16
Q

The relative charges of the electron, neutron, and proton, in that order.

A

-1, 0, +1

17
Q

J.J. Thomson’s cathode ray tube experiment led to the discovery of which subatomic particle?

A

The electron

18
Q

If a sample of thiourea (CH4N2S) contains 2.91 x 1018 molecules, how many moles is this equal to?

A
19
Q

What is the mass of 6.90mol of Iridium?

A
20
Q

In the hyphen notation carbon-12, the 12 represents this.

A

The mass number

21
Q

The center of an atom, composed of protons and neutrons.

A

Nucleus

22
Q

The atom that was chosen as the standard for the relative atomc mass scale.

A

Carbon-12

22
Q

What parts of Dalton’s atomic theory are now known to be incorrect?

A
  1. Atoms are not indivisible (they are composed of smaller particles).
  2. All atoms of a given element are not necessarily identical (many elements have isotopes).
23
Q

How many hydrogen atoms are there in 4.50mol of diammonium phosphate, (NH4)2HPO4?

A
25
Q

A law that states “mass is neither created nor destroyed during ordinary chemical reactions or physical changes.”

A

The Law of Conservation of Mass

26
Q

If a sample of silver contains 5.97 x 1024 atoms, how many moles are there?

A
28
Q

Selenium has five different stable isotopes. Using the data below, calculate that average atomic mass of selenium to two decimal places.

     Nuclide     Isotopic Mass     %Abundance

Se-74 73.922amu 0.89%

Se-76 75.919amu 9.37%

Se-77 76.920amu 7.63%

Se-78 77.917amu 23.77%

Se-80 79.917amu 49.61%

Se-82 81.912amu 8.73%

Note: You may have to stop in the middle of the calculation, press equals, and then continue.

A

(73.922u x 0.0089) + (75.919u x 0.0937) + (76.920u x 0.0763) + (77.917u x 0.2377) + (79.917u x 0.4961) + (81.912u x 0.0873) = 78.96u

29
Q

The number of protons in the nucleus of an atom is given by this number.

A

The atomic number (Z).

31
Q

This negatively charged, smallest subatomic particle is about 1,836 times lighter than the other two subatomic particles.

A

Electron

32
Q

How many molecules of carbon monoxide would there be in 3.8mmol?

A
34
Q

Complete the table:

A
35
Q

What did Robert A. Millikan’s oil drop experiment allow scientists to determine?

A

The mass of the electron

36
Q

How many oxygen atoms in NaNO3? How many in Ca(NO3)2 ? How many in Al(NO3)3? What is the general rule for counting atoms in parentheses?

A

3, 6, 9; multiply the subscript outside the parentheses by the subscripts inside the parentheses.

37
Q

Ernest Rutherford’s gold foil experiment gave experimental evidence suggesting that atoms have these.

A

Nuclei

38
Q

A law that states “if two or more different compounds are composed of the same two elements, then the ratio of the masses of of the second element combined with a certain mass of the first element is always a ratio of small whole numbers.”

A

The Law of Multiple Proportions

39
Q

A positively charged subatomic particle, found in the nucleus of an atom.

A

Proton

40
Q

Atoms of the same element having a different number of neutrons.

A

Isotopes

41
Q

The weighted mass of all the naturally occurring isotopes of an element.

A

Average atomic mass

Chemistry (13 decks)

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