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Chemistry > Exam 1 chem 1200 > Flashcards

Exam 1 chem 1200 Flashcards

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1
Q

Who Proposed that at the same temperature and pressure, equal volumes of different gases contain the same number of particles?

A

Amadeo Avogadro

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2
Q

Particles found in the nucleus of an atom

A

Protons

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3
Q

A set of hypothesis that attempts to explain a natural phenomenon

A

Theory

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4
Q

The fundamental SI unit for length

A

Meters

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5
Q

nano——n

A

10^-9

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6
Q

micro

A

10^-6

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7
Q

milli——m

A

10^-3

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8
Q

centi—-c

A

10^-2

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9
Q

deci—–d

A

10^-1

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10
Q

deca—-da

A

10^1

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11
Q

hecto—h

A

10^2

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12
Q

kilo—–k

A

10^3

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13
Q

mega—M

A

10^6

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14
Q

SI Fundamental unit for time?

A

second

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15
Q

SI Fundamental unit for mass?

A

kilogram

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16
Q

SI Fundamental unit for Temp?

A

kelvin

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17
Q

SI Fundamental unit for Electrical current?

A

ampere

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18
Q

SI Fundamental unit for amount?

A

mole

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19
Q

1 decameter^3 is = to ?L

A

1

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20
Q

1 ml is = to how many cc?

A

1

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21
Q

Definition:

Agreement of a particular value with the true value

A

Accuracy

22
Q

Definition:

Degree of agreement among several measurements of the same quantity.

A

Precision

23
Q

Nonzero integers always count as significant figures

how many sig figs in 4563?

A

4

24
Q

Leading zeros are zeros that precede all the nonzero digits. These do not count as significant figures
how many sig figs in 0.031?

A

2

25
Q

Captive zeros are zeros between nonzero digits. These always count as significant figures
How many sig figs in 41.04?

A

4

26
Q

Trailing zeros are zeros at the right end of the number. They are significant only if the number contains a decimal loin
How many sig figs are in examples 1 and 2?
1— 2.400
2–700

A

1- 4 sig figs

2-1 sig fig

27
Q

1 inch is equal to how many cm?

A

2.54cm

28
Q

How do you calculate sig figs in multiplication/division?

A

For multiplication or division, the number of significant figures in the result is the same as the number in the least precise measurement used in the calculation

29
Q

how do you calculate sig figs in +/-?

A

For addition or subtraction, the result has the same number of decimal places as the least precise measurement used in the calculation

30
Q

what has visibly indistinguishable parts; solution.

A

homogenous mixture

31
Q

what has visibly distinguishable parts?

A

heterogenous mixture

32
Q

Change in the form of a substance, not in its chemical composition…Can be used to separate a mixture into pure compounds, but it will not break compounds into elements

A

Physical Change

Example: boiling or freezing water

33
Q

A given substance becomes a new substance or substances with different properties and different composition

A

Chemical Change

Example: Bunson Burner

34
Q

Who: Element: A substance that cannot be broken down into simpler substances. AKA the father of Modern Chem

A

Robert Boyle

35
Q

Definition: Atom

A
  • Matter is composed of tiny particles called atoms.

* Atom:smallest part of an element that is still that element.

36
Q

Definition: One substance changes to another by reorganizing the way the atoms are attached to each other

A

A Chemical Reaction

37
Q

what is Process that lies at the center of scientific inquiry?

A

The Scientific Method

38
Q

Which law states Mass is neither created nor destroyed in a chemical reaction

A

Law of conservation of mass (Lavoisier)

39
Q

Which law states A given compound always contains exactly the same proportion of elements by mass

A

Law of definite proportion (Proust)

40
Q

What is the Law of multiple proportions?

A

When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers

41
Q

Who: Each element is made up of tiny particles called atoms
The atoms of a given element are identical;
the atoms of different elements are different in some fundamental way or ways

A

Dalton

42
Q

Who: Chemical compounds are formed when atoms of different elements combine with each other. A given compound always has the same relative numbers and types of atoms
-Chemical reactions involve reorganization of the atoms—changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction.

A

Dalton

43
Q

Who: Measured (under same conditions of T and P) the volumes of gases that reacted with each other.

A

Gay—Lussac

44
Q

Who: At the same T and P, equal volumes of different gases contain the same number of particles.

A

Avogadro

45
Q

Who: Postulated the existence of electrons using cathode-ray tubes.
Determined the charge-to-mass ratio of an electron.
The atom must also contain positive particles that balance exactly the negative charge carried by particles that we now call electrons.
Pllum pudding model

A

JJ Thomas

46
Q

Who: Performed experiments involving charged oil drops.
Determined the magnitude of the charge on a single electron.
Calculated the mass of the electron. 9.11 x 10-31 kilograms

A

Robert Millikan

47
Q

Who: Explained the nuclear atom.
Atom has a dense center of positive charge
called the nucleus.
Electrons travel around the nucleus at a relatively large distance

A

Ernest Rutherford (1911)

48
Q

Definition: Isotopes

A

Atoms with the same number of protons but different numbers of neutrons.
Show almost identical chemical properties; chemistry of atom is due to its electrons.
In nature most elements contain mixtures of isotopes.

49
Q

A certain isotope X contains 23 protons and 28 neutrons.

• What is the mass number of this isotope? • Identify the element.

A

Mass Number = 51 Vanadium

50
Q

What is a Mole?

A

Mole – a unit for counting atoms and molecules

1 mole = 6.022×1023

Chemistry (2 decks)

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