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Chemistry 1210 > Basics > Flashcards

Basics Flashcards

(66 cards)

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1
Q

Differentiate between the three states of matter

A

Solids have shape, a defined volume, and are not compressible
Liquids have no shape, a defined volume and are not compressible
Gases have no shape or volume, will assume shape and volume of container and are easily compressible

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2
Q

Define Chemistry

A

the study of matter, its properties, and the mechanisms involved in its changes

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3
Q

Define Matter

A

Any substance that has mass and occupies space

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4
Q

Atoms

A

Fundamental building blocks of matter which cannot be broken down into smaller units

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5
Q

Pure substance

A

one specific arrangement of atoms/molecules and cannot be physically separated

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6
Q

Element

A

a pure substance made up of only one type of atom that cannot be chemically decomposed

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7
Q

Compound

A

a pure substance made up of multiple types of atoms that can be chemically decomposed

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8
Q

Mixtures

A

Contain more than one compound

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9
Q

homogeneous mixtures

A

uniform consistency, regularly distributed

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10
Q

heterogeneous mixtures

A

non-uniform consistency

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11
Q

physical properties

A

traits that can be expressed without requiring a change in chemical composition or identity

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12
Q

chemical properties

A

traits that can be expressed only after a change in chemical composition has occurred

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13
Q

physical changes

A

transformations that do not involve a change in chemical composition and can easily be undone

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14
Q

chemical changes

A

atoms and molecules get redistributed and end up in a different combination than when started

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15
Q

Scientific Method

A

Observe problem
Make educated guess (hypothesis)
Run Tests if wrong guess again
Make general statement

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16
Q

law

A

a conceptual or mathematical statement about what is observed in nature that has been proven true

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17
Q

theory

A

neither been proven nor disproven and attempts to explain the underlying cause

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18
Q

mass

A

amount of matter in a substance

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19
Q

temperature

A

a measurement of the kinetic energy of molecules inside a sample

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20
Q

heat

A

a transfer of energy due to a temperature difference

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21
Q

Volume (SI)

A

1 cm3 = 1 cc = 1 mL

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22
Q

Unit Conversion larger to smaller prefix

A

Answer is always larger

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23
Q

Unit Conversion smaller to larger prefix

A

Answer is always smaller

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24
Q

Conversion factor

A

the prefix multiplier always goes with the prefixless base unit

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25
Accuracy
how close you got to a known, accepted value (bullseye)
26
Percent error
a commentary on the accuracy of your measurement
27
Sig Fig rules
All nonzero digits are significant Zero is significate if it between nonzero digits or is trailing Zero is not significant if it comes at the end of number without a decimal or at beginning of a number
28
Moore's Law
The number of transistors in an integrated circuit doubles approximately every eighteen months.
29
John Dalton (1808)
Matter consists of atoms, which are the smallest identifiable unit of matter and cannot be destroyed. All atoms of the same element are identical to each other, but are different than atoms of another element. Atoms combine in small whole number ratios when formin compounds
30
Law of Conservation of Matter
Matter can neither be created nor destroyed
31
Law of multiple Proportions
When an element combines with a different element to form multiple compounds, that ratio of the masses of one element to a fixed amount of the second element is a ratio of small whole numbers
32
Law of Definite Proportions
The same compound will always be comprised of its constituent elements in the same proportion by mass
33
J. J. Thompson (1897)
Crooke's tube, cathode ray, deflected by electric field, suggest negative particles. Using magentic field negatively particles deflected. Based on strength applied he balanced out the opposing defelction. He calculated mass-to-charge ratio
34
Robert Millikan (1909)
X-ray remove electrons from air molecules. Oil drop pick up electrons. Oil became charged. Millikan measure mass in electric field and out. Mass of a electron 9.109E-28grams
35
Thompson model (plum-pudding)
atom spherical void of positive charge, with electrons uniformly embedded in volume
36
Rutherford's Gold Foil (1911)
A beam of positively charged particles (alpha) was directed at a thin piece of gold foil. Like positive atoms repel each other. Positively charged nucleus -The area had to be positively charged to deflect positively charged α-particles. Additionally, the area had to be relatively massive to physically intersect the incident energy beams, yet small enough to account for the observation that the majority of alpha rays went straight through.
37
Why gold?
Its ability to be formed into very thin sheets (malleability)
38
James Chawick (1932)
Neutron
39
Atomic number
number of protons
40
Ion
number of electrons and protons are not equal, an atom loses it neutrality and adopts an overall charge
41
Cations
positively charged ions
42
Anions
negatively charged ions
43
Isotopes
atoms of the same element with a different number of neutrons
44
Atomic Mass
weighted average of all the elements naturally occurring isotopes
45
Periodic Law
rationale for the organization of the elements
46
Dmitri Mendeleev (1864)
periodic table
47
Periodic table
Rows - (periods) | Columns -(groups)
48
Metalloids
semimetals
49
Malleable
can be formed into thin sheets
50
Ductile
can be pulled into thin wire
51
Lustrous
shiny
52
Metal characteristics
Malleable, ductile, lustrous, heat and electric conductors, large densities, high melting and boiling, solid at room temp (except Hg), form cations, few colors
53
Nonmetal characteristics
Brittle, dull, insulator, low density, melting and boiling, various states at room temp, form anions, variety color
54
Metalloids
have intermediate characteristics of metals and nonmetals. Semiconductors
55
Alkali metals
soft, low density, react violently with water
56
Alkaline earth metals
harder, higher desity and melting less reactive to water.
57
Halogens
found paired with an identical atoms. very reactive and have a tendency to react with metals to form salts
58
Noble gases
Inert
59
Avogadro’s Number
1 mole (mol) = 6.022 × 1023 individual units
60
Molar mass
the mass in grams of exactly 1 mole of a substance grams/1mol or 1mol/grams
61
Relationship between wavelength and frequency
The speed of light is fixed. Therefore, as wavelength decreases, the frequency must increase to maintain the constant. Hence, these values are inversely proportional.
62
diffraction pattern
A typical pattern consists of bands of alternating intensity
63
Rydberg equation
ya
64
Rayleigh–Jeans Law
as temperature increases so does energy density
65
Planck (1900)
electron oscillators of a blackbody absorbed and emitted energy only in small, discrete packets, called quanta. Furthermore, each quantum had an energy that was directly proportional to its frequency:
66
photoelectric effect
when a metal absorbs sufficient energy, its electrons can be ejected from the surface with a measurable velocity

Chemistry 1210 (3 decks)

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