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Chemisty Honors > Unit 1: Into and Atomic Theory > Flashcards

Unit 1: Into and Atomic Theory Flashcards

1
Q

Scientific Method

A

Ask a question, do background research, construct a hypothesis, experiment, analyze data, make a conclusion

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2
Q

Qualitative Data

A

Involves observations, words and descriptions of observations

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3
Q

Quantitative Data

A

Involves measurements, number

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4
Q

SI units (length)

A

meter (m), tool to measure is ruler/meter stick

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5
Q

SI units (mass)

A

kilograms (kg), tool to measure balance

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6
Q

SI units (time)

A

seconds (s), tool to measure is clock/stopwatch

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7
Q

Metric Prefixes (H)

A

hecto, 10^2 base

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7
Q

Metric Prefixes (K)

A

kilo, 10^3 base

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8
Q

SI units (temperature)

A

kelvin (k), tool to measure is thermometer

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8
Q

SI units (amount of substance)

A

mole (mol), no tool of measure

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9
Q

derived unit

A

combination of basic SI units (density, volume)

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10
Q

Metric Prefixes (D)

A

deka, 10^1 base

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11
Q

Metric Prefixes (base)

A

meter, liter, gram, second

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12
Q

Metric Prefixes (d)

A

deci, 10^-1 base

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13
Q

Metric Prefixes (c)

A

centi, 10^-2 base

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14
Q

Metric Prefixes (m)

A

milli, 10^-3 base

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15
Q

Metric Prefixes (u)

A

micro, 10^-6 base

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16
Q

Metric Prefixes (n)

A

nano, 10^-9 base

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17
Q

Metric Prefixes (p)

A

pico, 10^-12 base

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18
Q

Metric System

A

1 cm^3 = 1 mL

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19
Q

Dimensional analysis

A

A method of problem-solving that focusis on the units used to describe matter (Metric Prefixes)

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20
Q

Significant Figures

A

Non-zero digits are always significant, any zero between sig figs are significant, any zero in front of non-zero digits aren’t significant, a final zero or trailing zeros in the decimal portion only are signifcant

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21
Q

Precision

A

How close a series of measurements are to each other (consistent/reproducible)

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21
Q

Significant Figures (add/subtract)

A

fewest amount of decimal places

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21
Q

Accuracy

A

How close a measurement is to the accepted value

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22
Q

Significant Figures (multiply/divide)

A

use the fewest number of sig figs

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23
Q

Percent Error

A

Percent Error = ( |experimental value - actual value| / actual value )*100

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24
Q

Systematic Errors

A

Affects all measurements taken (ex. forgetting to calibrate a balance/scale)

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24
Q

Personal Errors

A

Never say “human error” (ex. not using proper or precise experiment; timing an experiment inconsistently)

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25
Q

Random Errors

A

Fluctuations in experimental/measurements (ex. not in stable conditions; physical/environmental errors)

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26
Q

What is the acceptable margin of error in science?

A

+/- 10%

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27
Q

Most common type of graph in chemistry?

A

Line graph

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28
Q

Density

A

A ratio that compares the mass of an object to its volume, D=M/V

29
Q

Atom

A

The fundamental unit of which elements are composed

30
Q

Structures of the atom

A

Proton, Neutron, Electron

30
Q

Compounds

A

Atoms of two or more elements chemically combined to make up a compound, compounds can be formula units or molecules

31
Q

Quarks

A

The atom consists of three subatomic particles (protons, neutrons, electrons), the electron is an elemental particle whereas the proton and neutron consist of three smaller particles called quarks

32
Q

Nucleons

A

Particles in the nucleus (protons and neutrons)

33
Q

Isotopes

A

Atoms of the same element with a different number of neutrons

34
Q

DEF

A

Average of all the masses of all the isotopes in an element’s sample, decimal value on periodic table

35
Q

Nuclides

A

A particular isotope of an element (C -12, C -14)

36
Q

Ion

A

An atom that has lost or gained an electron, lost electron: positive charge, gained electron: a negative charge

37
Q

Uses of Mass Spectrometry

A

Identify isotopes and the relative abundance of each isotope in nature

37
Q

Average Atomic Mass

A

AAM = (mass number * percentage abundance) + (mass number * percentage abundance)

38
Q

Mass Spectrometry

A

A device that separates positive gaseous ions according to their mass to charge ratio (mass for +1 ions)

39
Q

Democritus

A

Came up with the word “atom”, Atomic theory: Atoms are solid and indestructible, different things contain different atoms, this theory would later be famously rejected

40
Q

John Dalton

A

Modern Atomic Theoyr: All matter is made up of atoms, all atoms of an elemen are identical, and different from atoms of other elements, atoms cannot be created, divided, or destroyed, law of multiple proportions

41
Q

Law of Multiple Proportions

A

Atoms combine in whole number ratios to form compounds, was created from his modern atomic theory

42
Q

JJ Thomson

A

Discovered electrons, developed the mass spectrometer, developed a model based off of his discoveries called the “Plum Pudding Model”

43
Q

James Chadwick

A

Discovered the neutron,

43
Q

Ernest Ruthford

A

Used the “Gold Foil Experiment” to discover protons and the nucleus, also determined that atoms are mostly made up of empty space, created “The nuclear model”

43
Q

Robert Millikan

A

Discovered the mass (9.1x10^-28g) and charge of an electron using the “oil drop experiment”

44
Q

What changes were made to Dalton’s Atomic Theory?

A

Atoms are not invisible, and indestructible; they are made up of smaller particles, atoms pf the same element aren’t exactly alike; they can have the same number of protons, but may have different numbers of neutrons

45
Q

Gold Foil Experiment

A

Shot alpha particles from a radioactive source at a thin sheet of gold foil, most of the particles passed straight through the foil, some deflected back, to the side, or at other angles, this concluded that atoms were mainly made up of empty space, and that atoms have a positively dense core called the nucleus

46
Q

Niels Bohr

A

Created the Bohr model or the atom, electrons move in specific circular orbits around the nucleus based on their energy levels

46
Q

Electron Cloud Model

A

Atoms are the smallest particle of an element that retains the physical properties of that element, the diameter of an atom is around 1x10^-10 m, atoms are composed of three subatomic particles (protons, neutrons, and electrons), the central part of an atom is called the. nucleus

47
Q

Nuclear Chemistry

A

The sub-field of chemistry dealing with the radioactivity, nuclear processes, and transformations of the nuclei of atoms, such as nuclear transmutation and nuclear properties

48
Q

Radioisotopes

A

The isotopes of an atom with unstable nuclei

49
Q

Transmutation

A

A change in the identity of an atom caused by a change in the number of protons

50
Q

Mass Defect

A

The difference between the mass of an atom and the sum of the masses of its protons, neutrons, and electrons

51
Q

What are the causes of Mass defect?

A

Some mass is converted to energy when the nucleus forms, this energy is called binding energy, as the nuclear binding energy increases, the stability of the nucleus increases

52
Q

Nuclear Reactions

A

In order to stabilize a nucleus, atoms release a tremendous amount of energy

53
Q

Nuclear Stability

A

The most stable nuclei have a neutron/proton a ratio of 1:1 to 1.5:1, elements within this range are considered to be in the “band of stability”

54
Q

Radioactive Decay

A

The spontaneous disintegration of a nucleus into a lighter, more stable nucleus with the emission of particles, electromagnetic radiation, or both

55
Q

Radioactive Nuclide

A

An atom that has excess nuclear energy making it unstable

56
Q

Alpha Particle Decay

A

Occurs in unstable heavy nuclei, number of protons and neutrons are decreased, 4/2 he

57
Q

Electron Capture

A

An inner orbital electron is captured by the nucleus, decreasing the number of protons and increasing the number of neutrons

57
Q

Half-life

A

The time required for a quantity to reduce to half of its initial value

57
Q

Beta Particle Decay

A

An electron is emitted from a nucleus in order to decrease the number of electrons and increase the number of protons (elements found above the band of stability)

57
Q

Fission

A

A nuclear reaction where the nucleus of a radioactive nuclide splits into two or more different atoms, releases energy, we harness this energy for nuclear power plants

57
Q

Positron Emission

A

A proton inside a radionuclide nucleus is converted into a neutron while releasing a positron

58
Q

Gamma Radiation

A

high energy, electromagnetic radiation is released from a nucleus as it goes from a unstable excited state to a more stable ground state, usually follows some other type of decay

59
Q

Parts of a nuclear reactor (fuel)

A

usually uranium-235 or plutonium-239, used to convert fission to heat

60
Q

Parts of a nuclear reactor (moderator)

A

Increases efficiency of reaction by slowing down fast moving neutrons

61
Q

Parts of a nuclear reactor (Control Rods)

A

Absorbs neutrons yo control the chain reaction; made of boron, cadmium, gadolinium

62
Q

Parts of a nuclear reactor (coolant)

A

heated by fission drives turbine; made of water, liquid, sodium, helium

63
Q

Fusion

A

A nuclear reaction where two or more nuclei combine to form a new atomic nuclei, releases or absorbs a lot of energy, this is what powers the sun

64
Q

Radioactive Dating

A

Approximates age of an object based on the presence of a radioactive nuclide with a known half-life, uses americium-241, ionizes air when the small electric current is blocked by alarm sounds

65
Q

Nuclear Agriculture

A

Tracers in fertilizers to monitor effectiveness, prolong shelf life

66
Q

Smoke Detectors

A

A radioactive gas that naturally occurs in the atmosphere, it is often found in basements and many homes undergo radon testing to decrease the level that inhabitants are exposed to

67
Q

Nuclear Medicine

A

Radioactive tracers (barium) uses yp find things like a blocked kidney, radiation therapy for cancer (colbalt-60), CAT scans show cross sectional views of the body, PET scans show images of the cellular function and biological function of the body, and the sterilization of medical instruments

Chemisty Honors (3 decks)

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