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Chem 100, Exam 1 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

What is a homogeneous mixture?

A

Homogeneous mixtures have uniform composition throughout

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2
Q

What is a heterogeneous micture?

A

heterogeneous mixtures do not have uniform composition throughout

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3
Q

What is John Dalton’s atomic theory?

A

-All matter is composed of small particles called atoms
-Atoms of a given element are identical in mass and properties
-Atoms of different elements have different masses and properties
-Atoms combine in simple whole-number ratios to form compounds
-Chemical reactions involve the rearrangement of atoms, not their creation or destruction

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4
Q

What are the 3 subatomic particles?

A

-Protons
-Neutrons
-Electrons

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5
Q

What is the mass of an element determined by?

A

The sum of protons and neutrons

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6
Q

What are covalent bonds?

A

Covalent bonds involve the sharing of electrons between atoms

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7
Q

What are hydrogen bonds?

A

Hydrogen bonds are intermolecular forces that occur between 2 water molecules

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8
Q

Why is water cohesive?

A

Due to hydrogen bonding

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9
Q

Is water polar?

A

Yes. It forms strong intermolecular bonds with itself

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10
Q

Is water a universal solvent?

A

Yes

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10
Q

Equation to get Celsius from Farenheit

A

C = (F-3)(5/9)

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11
Q

T/F: Exact numbers limit the number of significant figures in a calculated result

A

False

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11
Q

What scales are used to measure temperature?

A

Farenheit, Celsius, Kelvin

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11
Q

What is temperature a measure of?

A

The kinetic energy of molecules

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11
Q

Does heat transfer from cold to hot, or hot to cold?

A

Heat always transfers from a hotter object to a colder one

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11
Q

Equation to get Farenheit from Celsius

A

F = (9/5)(C) + 32

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12
Q

Equation to get temperature in Kelvin from Celsius

A

K = C+273

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12
Q

What is the Law of Constant Composition (Definite Proportions)?

A

All samples of a pure compound contain the same elements in the same proportion by mass

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12
Q

T/F: The composition of compounds always consistent, regardless of how or where they are formed

A

True

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13
Q

What do significant figures always include?

A

-Nonzero digits
-Captive zeros
-Trailing zeros (when right to decimal point, when in scientific notation)

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14
Q

What do significant figures not always include?

A

-Leading zeros
-Trailing zeros (when left to a decimal point)

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15
Q

When multiplying/dividing, is the answer rounded to the smallest number of decimal places, or the smallest number of sig figs?

A

The smallest number of sig figs

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16
Q

When adding/subtracting, is the answer rounded to the smallest number of decimal places, or the smallest number of sig figs?

A

The smallest number of decimal places

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17
Q

What is the density formula?

A

d = (m/v)

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18
Q

What can density be used for?

A

Density can be used to determine whether an object will float or sink in a liquid

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19
Q

What did J.J. Thompson experiment with?

A

Cathode ray tubes

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20
Q

What did J.J. Thompson’s experiments lead to?

A

The discovery that atoms contain small, negatively charged particles called electrons. No matter what the metal was, the cathode ray tubes would get the same results (deflected towards the positive plate)

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21
Q

T/F: Electrons are heavier than atoms

A

False. Electrons are way lighter than atoms.

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22
Q

What did Millikan experiment with?

A

oil drops

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23
Q

What did Millikan’s experiments lead to?

A

The discovery that there is a fundamental electric charge (the charge of the electron)

24
Q

What was the oil drop charge in Millikan’s experiments?

A

1.6 x 10^-19

25
Q

What is the mass of the electron?

A

9.10 x 10^-31 kg

26
Q

What did Rutherford Experiment with?

A

Gold Foil

27
Q

What were the results of Rutherford’s experiments?

A

Atoms have a small, dense, positively charged nucleus; the positively charged particles within the nucleus are called protons (a - alpha particles are positively charged)

28
Q

Do protons, neutrons, or electrons occupy most of the atom’s volume?

A

Electrons

29
Q

T/F: Samples that have the same mass ratio are not necessarily the same substance

A

True

30
Q

What is the Law of Multiple Proportions?

A

When two elements react to form more than one compound, a fixed mass of one element will react with masses of the other element in a ratio of small, whole numbers

31
Q

What subatomic particles are located in the nucleus?

A

Protons and neutrons

32
Q

What are isotopes?

A

Atoms of the same element with different masses

33
Q

Who were neutrons discovered by?

A

James Chadwick

34
Q

T/F: The nucleus contains almost all the mass of an atom

A

True

35
Q

What is the diameter of an atom?

A

10^-10

36
Q

What is the diameter of the nucleus

A

10^-15

37
Q

Greek prefix - Centi

A

1 x 10^-2

38
Q

Greek prefix Milli:

A

1 x 10^-3

39
Q

Greek prefix Micro

A

1 x 10^-6

40
Q

Greek prefix Nano

A

1 x 10^-9

41
Q

Greek prefix Pico

A

1 x 10^-12

42
Q

What is the speed of light?

A

c = 2.998 x 10^8 m/s

43
Q

What is the relationship between wavelength and frequency?

A

Wavelength and frequency are inversely proportional. As one increases, the other decreases

44
Q

What is wavelength?

A

The distance between two consecutive peaks of a wave

45
Q

What is frequency?

A

The number of wavelengths that pass a given point per unit time, measured in Hertz (Hz)

46
Q

What is the equation for the relationship between wavelength and frequency?

A

c=λν

47
Q

What is amplitude?

A

Amplitude is the height of the wave from its midpoint to its peak or trough. (Related to the energy and intensity of the wave)

48
Q

T/F: Amplitude is related to the frequency or wavelength of a wave

A

False

49
Q

What is the order of the electromagnetic spectrum, from longest wavelength/lowest frequency to shortest wavelength/highest frequency?

A

Radio waves, microwaves, infrared, visible light, ultraviolet, x-rays, gamma rays

50
Q

T/F: Visible light is a small part of the electromagnetic spectrum

A

True

51
Q

What is the relationship between energy and frequency?

A

Energy and frequency are directly proportional. Higher frequency waves have higher energy

52
Q

What is the equation for energy?

A

E = hv

53
Q

What is Planck’s constant?

A

(6.626 x 10^-34 Js)

54
Q

What is the photoelectric effect?

A

The photoelectric effect occurs when light of a certain frequency hits a metal surface and ejects electrons

55
Q

What is blackbody radiation?

A

The emission of light from an idealized object that absorbs all incident radiation. This spectrum depends on the temperature of the object

56
Q

What is spectroscopy?

A

The study of the interaction between light and matter

57
Q

T/F: Electrons move from ground state to excited state due to electricity

A

True

58
Q

When does emission of photons occur?

A

When electrons return to the ground state from the excited state

59
Q

What is continuous spectra?

A

Produced by dense materials, unbroken series of wavelengths

60
Q

What is line spectra?

A

Produced by gases at low pressure, narrow line widths.

61
Q

What is the Rydberg equation?

A

look at notes

62
Q

What is the Bohr model?

A

It introduced the concept of quantized orbits for electrons, where electrons do not emit radiation. Explained the line spectra of hydrogen

63
Q

What is the difference between physical change and chemical change?

A

Physical change alters the form or appearance of a substance without changing its chemical composition. In a chemical change, the kind of matter changes and at least one new substance with new properties is formed.

64
Q

Examples of physical change

A

Melting ice to water, boiling water, freezing water

65
Q

Examples of chemical change

A

Burning wood, cooking, rusting, rotting

66
Q
A

Chem 100, Exam 1 (1 decks)

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