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PB Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What are the symbol and the charge of a proton?

A

p+, positive charge

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2
Q

Protons and neutrons have this mass in grams and this mass in amu:

A

1.67 x 10^-24 g

1 amu

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3
Q

Protons and neutrons are found…

A

In the nucleus

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4
Q

Electrons are found…

A

In the electron cloud

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5
Q

Symbol and charge for neutrons

A

n0, 0 (zero charge)

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6
Q

Symbol and charge for electrons

A

e-, negative charge

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7
Q

Mass in g and amu for electrons

A

9.11 x 10^-28 g, 0 amu

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8
Q

The atomic number identifies…

A

The element.

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9
Q

The atomic number is equal to…

A

The number of protons in the nucleus.

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10
Q

When is the atomic number equal to the number of electrons?

A

When the atom is electrically neutral (no electrical charge).

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11
Q

What does the atomic mass represent?

A

The total number of protons and neutrons combined.

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12
Q

What are isotopes?

A

Atoms of the same element with the same atomic number but different atomic masses due to a different number of neutrons.

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13
Q

What are ions?

A

Atoms with a different number of electrons, meaning they have an electrical charge that is either positive or negative.

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14
Q

How do you calculate average atomic mass?

A

Convert the percentage of the sample to a decimal. Multiply each atomic mass by its corresponding decimal, and then add all of those products together.

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15
Q

With average atomic mass, how should you round and use sig figs?

A

Keep the number of decimal places in your answer consistent with the number of places in the given masses.

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16
Q

What is a mole in chemistry?

A

It is a counting unit.

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17
Q

What is the definition of a mole?

A

A mole is the amount of a substance that contains the same number of particles as there are in exactly 12 grams of Carbon-12.

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18
Q

How many particles are there in exactly 12g of Carbon-12?

A

6.022 x 10^23 particles

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19
Q

What particles make up elements?

A

Atoms

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20
Q

What particles make up compounds?

A

Molecules

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21
Q

The number 6.022 x 10^23 is also known as…

A

Avagadro’s Number.

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22
Q

In all elements, one mole of that element is equivalent to… (for grams)

A

The average atomic mass.

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23
Q

1 mole of Carbon-12 equals how many Carbon-12 atoms?

A

6.022 x 10^23 atoms.

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24
Q

1 mole of Carbon-12 equals how many grams of Carbon-12?

A

12.01 (the average atomic mass of Carbon 12).

25
Q

1 mole Cr=___g of Cr?

A

1 mole of Cr= 52.00 g of Cr (which is the average atomic mass of Cr).

26
Q

__mole=___atoms=___g

A

1 mole= 6.022 x 10^23 atoms= Avg. atomic mass of the element in grams

27
Q

What is the metric system unit for substance quantity?

A

Mole (mol)

28
Q

What is a representative particle?

A

The smallest unit in which a substance naturally exists.

29
Q

What is the representative particle for an ionic compound?

A

The formula unit.

30
Q

What is the representative particle for an element?

A

The atom.

31
Q

What is the representative particle for a compound?

A

The molecule.

32
Q

What does an ion symbol show?

A

It tells what an ion’s charge is.

33
Q

What does this ion symbol mean?

Cl-2

A

It is a chlorine atom with a charge of negative 2 meaning it has two more electrons than protons.

34
Q

What is the atomic mass of the isotope calcium-40? How many neutrons, protons, and electrons does it have? It is atomic number 20.

A

Mass: 40
Neutrons: 20
Protons: 20
Electrons: 20

35
Q

Calcium-40 is an…

A

Isotope.

36
Q

What does the “40” represent in the isotope name “calcium-40”?

A

The atomic mass.

37
Q

How do you label atomic mass?

A

…amu

Mass number, amu

38
Q

To convert from atoms to mass, what pathway must you use?

A

Atoms to moles to mass (grams).

39
Q

Given that the average atomic mass of Calcium is 40.08, what is the mass of 1.05 x 10^23 atoms of calcium?. Show the setup.

A

(1.05 x 10^23 atoms Ca/1)(1 mole Ca/6.022 x 10^23 atoms Ca)(40.08 g Ca/1 mole Ca)= 6.99 g

40
Q

The average atomic mass of any element is equivalent to what two things?

A

Avg. atomic mass= 1 mole of that element = 6.022 x 10^23 atoms of that element.

41
Q

The average atomic mass of carbon is 12.01, and the average atomic mass of oxygen is 16.00. What is the mass of one mole of CO2? How do you find this?

A

CO2= 1 carbon, 2 oxygen.
1(12.01) + 2(16.00)= 44.01. So the mass of one mole CO2 (or 6.022 x 10^23 molecules CO2) is 44.01 grams. (You could say, “The molar mass is 44.01.”)

42
Q

The average atomic mass of carbon is 12.01, and the average atomic mass of oxygen is 16.00. The mass of one mole CO2 is 44.01. What is the percent composition of carbon? Oxygen? How do you find this?

A

(part/whole) x 100. So if total molar mass CO2=44.01, divide the part by this number. (12.01/44.01) x 100= 27.29% carbon. (32.00/44.01) x 100=72.71% oxygen. (Since there are two oxygen atoms, you need to first multiply 16.00 x 2=32.00.)

43
Q

Who proposed atomic theory?

A

Dalton.

44
Q

Who theorized that all matter is made of tiny, invisible, uncuttable particles?

A

Dalton (and Democritus).

45
Q

Who discovered the negatively-charged electron?

A

Thomson.

46
Q

Who proposed the plum pudding atomic model, in which the atom was equally dense throughout?

A

Thomson.

47
Q

Who proposed the planetary atomic model?

A

Rutherford.

48
Q

Who discovered the atomic nucleus (and created a model including his discovery)?

A

Rutherford.

49
Q

Who created an atomic model named after himself?

A

Bohr.

50
Q

Who discovered the mass of an electron?

A

Millikan.

51
Q

Who discovered the charge-to-mass ratio of an electron?

A

Millikan.

52
Q

Who gave fundamental particles the name “atom”?

A

Democritus.

53
Q

What is Millikan known for?

A

Discovering mass and charge-to-mass ratio of an electron.

54
Q

What is Dalton known for?

A

Proposing his atomic theory and theorizing that all matter is made of tiny, invisible, uncuttable particles.

55
Q

What is Democritus known for?

A

Naming the fundamental particles “atoms” and theorizing that all matter is made of tiny, invisible, uncuttable particles.

56
Q

What is Thomson known for?

A

Discovering the negatively-charged electron and proposing the plum pudding model.

57
Q

What is Bohr known for?

A

Developing the Bohr model of the atom (an improvement from Rutherford’s planetary model).

58
Q

What is Rutherford known for?

A

Discovering the atomic nucleus and developing the planetary model.

PB Chemistry (9 decks)

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