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Chem-109 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Scanning tunneling microscopy (STM)

A

a technique that can image, and even move, individual atoms and molecules

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2
Q

tunneling current

A

the electrical current that flows between the tip of the electrode and the surface even though the two are not in physical contact

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3
Q

The smalles identifiable unit of an element

A

atom

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4
Q

the law of conservation of mass

A

In a chemical reaction, matter is neither created nor destroyed

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5
Q

Antoine Lavoisier formulated this law

A

the law of conservation of mass

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6
Q

Joseph Proust observed this law

A

The law of definite proportions

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7
Q

the law of definite proportions

A

All samples of a given compound, regardless of their source or how they are prepared, have the same proportions of their constituent elements

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8
Q

John Dalton stated this law

A

the law of multiple proportions

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9
Q

the law of multiple proportions

A

When two elements (A and B) form two different compounds, the masses of element B that combine with 1g of element A can be expressed as a ratio of small whole numbers.

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10
Q

John Dalton stated this theory

A

atomic theory

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11
Q

Atomic theory

A
  1. each element is composed of tine, indestructible particles called atoms
  2. all atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements
  3. atoms combine in simple, whole-numbered ratios to form compounds
  4. atoms of one element cannot change into atoms of another element.
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12
Q

J.J. Thompson used this to discover electrons

A

cathode rays in a cathode ray tube

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13
Q

electron

A

negatively charged, low mass partical present within all atoms

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14
Q

electrostatic forces

A

electrical charge is a fundamental property of some of the particles that compose atoms and results in attractive and repulsive forces

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15
Q

electric field

A

An area around a charged particle where electrostatic forces exist

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16
Q

J.J. Thompson discovered this

A

Electrons

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17
Q

Robert Millikan

A

discovered the charge of a single electron with his oil drop experiment

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18
Q

Electron charge

A

-1.60 x 10^-19 C

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19
Q

Electron mass

A

.00091 x 10^-27 kg

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20
Q

Radioactivity

A

the emission of small energetic particles from the core of certain unstable atoms

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21
Q

Henri Becquerel and Marie Curie discovered this

A

radioactivity

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22
Q

Rutherford proposed this

A

nuclear theory, after completing his gold foil experiment

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23
Q

nuclear theory states

A
  1. Most of the atom’s mass and all of its positive charge are contained in a small core called the nucleus
  2. most of the volume of the atom is empty space, throught which tine, negatively charged electrons are dispersed
  3. there are as many negatively charged electrons outside of the nucleus as there are positively charged particals withing the nucleus, so the atom is electrically neutral
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24
Q

neutrons

A

neutral particles withing the nucleus, with mass similar to a proton

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25
Q

James chadwick found these

A

neutrons

26
Q

Atomic Mass Unit (AMU)

A

defined as 1/12 the mass of a carbon atom containing six protons and six neutrons

27
Q

proton mass

A

1.672 x 10^-27 kg

28
Q

proton charge

A

+1.602 x 10^-19 C

29
Q

neutron mass

A

1.674 x 10^-27 kg

30
Q

neutron charge

A

0

31
Q

Defines an element

A

the number of protons

32
Q

atomic number

A

the number of protons in an element

33
Q

chemical symbol

A

one or two letter abbreviation listed directly below its atomic number

34
Q

Elements chemical symbols and names come from

A

English names, latin names, names to reflect properties, and astronomical bodies, and scientist who discovered it

35
Q

Isotope

A

Atoms with the same number of protons but different numbers of neutrons

36
Q

Natural abundance

A

the percentage of the individual isotopes found in nature

37
Q

mass number

A

the sum of the number of neurons and protons in an atom

38
Q

Ions

A

When an atoms loses or gains and electron

39
Q

Cation

A

positively charged ion

40
Q

anion

A

negatively charged ion

41
Q

Dmitri Mendeleev

A

created the periodic table, and stated the periodic law

42
Q

periodic law

A

When elements are arranged in order of increasing mass, certain sets of properties recur periodically

43
Q

Classifications of elements in the periodic table

A

metals, nonmetals, metalloids

44
Q

metals

A

lie on the lower left side and middle of the periodic table and share some common properties. good conductors, malleability, ductility, often shiny, and tend to lose electrons when they undergo chemical changes

45
Q

nonmetals

A

lie on the upper right side of the periodic table. varied properties(solid, liquid, gas), tend to be poor conductors, and they tend to gain electrons when they undergo chemical changes.

46
Q

metalloids

A

lie alone the zigzag diagonal line that divides metals and nonmetals. exhibit mixed properties. some are classified as semiconductors

47
Q

semiconductors

A

The classification for several metalloids, because of their intermediat and highly temperature dependent electrical conductivity. the ability to change and control conductivity makes them useful in making electronic chips and circuits.

48
Q

main group elements

A

properties tend to be largely predictable based on their position in the periodic table. 1a-2a, 3a-8a

49
Q

transition elements or transition metals

A

properties tend to be less predictable based on their position in the periodic table. 3b-8b, 1b-2b

50
Q

family or group

A

each column within the main-group regions of the periodic table

51
Q

Noble gasses

A

mostly unreactive, 8a

52
Q

alkali metals

A

reactive metals, 1a

53
Q

alkaline earth metals

A

fairly reactive, although not as reactive as alkali metals, 2a

54
Q

halogens

A

very reactive nonmetals, 7a

55
Q

Predicting ions (2 ways)

A
  1. main group metal tends to lose electrons, forming a cation with the same number of electrons as the nearest noble gas
  2. main group nonmetals tend to gain electrons, forming an anion with the same number of elctrons at the nearest noble gas
56
Q

Atomic mass

A

calculation of the average mass of an element found by taking the percent natural abundance found of each isotope.

57
Q

Mole

A

the amount of a material containing 6.022 x 10^23 particles

58
Q

avogadros number

A

6.022 x10^23 particles,

59
Q

How does the mole get its specific value

A

the value of the mole is equal to the number of atoms in exactly 12 grams of pure carbon-12

60
Q

1 mole = (particles, grams)

A

6.022 x 10^23 particles, atomic mass # of grams

61
Q

molar mass

A

an element’s molar mass in grams per mole is numerically equal to the element’s atomic mass in atomic mass units

Chem-109 (12 decks)

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