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Notes Taken 3 Flashcards

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Biology 101 flashcards
1
Q

Too small to be seen even with the aid of the very best of microscopes.

A

Microscopic

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2
Q

Attractive forces that hold particles together

A

Intramolecular forces

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3
Q

The force of attraction between identical molecules

A

Cohesion

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4
Q

The force of attraction between different molecules

A

Adhesion

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5
Q

Ability to flow

A

Fluidity

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6
Q

Resistance to flow

A

Viscosity

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7
Q

The energy required to increase the surface area of a liquid by a given amount

A

Surface tension

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8
Q

Compounds that lower the surface tension of water

A

Surfactants

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9
Q

SI unit for pressure

A

Pascal

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10
Q

Used to measure pressure

A

Barometer

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11
Q

Discovered Radium and Polonium

A

Marie Curie and Pierre Curie

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12
Q

Metal that Has the highest melting point

A

Tungsten

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13
Q

Most abundant element in the universe

A

Hydrogen

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14
Q

Substances whose colors are affected by acids and bases

A

Indicators

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15
Q

The random movement of microscopic particles suspended in a liquid or gas, caused by collisions with molecules of the surrounding medium.

A

Brownian movement

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16
Q

Properties that can be observed by the five human senses, aided or unaided

A

Macroscopic

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17
Q

The metalloids

A

Boron, Silicon, Arsenic, Antimony, Tellurium Germanium

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18
Q

Used as as a quick way to show the composition of compounds

A

Chemical formula

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19
Q

Formula for density

A

p= Mass/Volume

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20
Q

The only nonmetal that is liquid

A

Bromine

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21
Q

Phase changes that Require energy

A

Melting, Vaporization, Sublimation

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22
Q

Phase changes that release energy

A

Condensation, freezing, deposition

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23
Q

The temperature where liquid is change into crystalline solid

A

Freezing point

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24
Q

Building blocks of matter that make up everything that exists in our world.

A

Atoms

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25
Q

First proposed that everything is composed of very small bit of matter that is indivisible and called it atom

A

Democitus and Leucippus

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26
Q

Explained the idea that like fluids repel and unlike attract. This idea helped in the development of the theory of absolute measurement

A

Charles-Agustin de Coulumb

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27
Q

Made a clarification on his concept of an element that it could not be broken down by any method of chemical analysis. He devised a theory of the formation of chemical compounds from elements

A

Antoine Lavoisier

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28
Q

Came up with the atomic theory

A

John Dalton

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29
Q

Constructed the forerunner of the modern television picture tube to investigate the properties of cathode rays

A

Sir William Crookes

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30
Q

Negative or positive: anion

A

Negative

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31
Q

Positive of negative: anode

A

Positive

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32
Q

Positive or negative: cation

A

Positive

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33
Q

Positive or negative: cathode

A

Negative

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34
Q

Discovered x-ray by observing the fluorescence they produced

A

Wilhelm Roentgen

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35
Q

Stated that radioactive materials cause atoms to break down spontaneously. As this happens, radiation is released in the form of energy and subatomic particles.

A

Pierre Curie and Marie Curie

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36
Q

Discovered the electron

A

Joseph John Thomson

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37
Q

Stated that energy is radiated in small, discrete units, which he called quanta

A

Max Planck

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38
Q

Created the special and general theories of relativity and hypothesized the particle nature of light.

A

Albert Einstein

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39
Q

Worked on atomic physics and major science, dealing with the basic constituents of the universe, the forces they exert on one another, and the results produced by these forces.

A

Robert Millikan

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40
Q

Worked on nuclear physics and invented a detector for electromagnetic waves

A

Ernest Rutherford

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41
Q

Proposed the planetary model of an atom. He also made numerous contributions on quantum mechanics.

A

Neils Bohr

42
Q

Discovered that electrons have a dual nature similar to both particles and waves-particle/wave duality

A

Louise De Broglie

43
Q

Explained how the electrons move in an atom as a wave

A

Erwin Schrodinger

44
Q

Discovered the neutron

A

James Chadwick

45
Q

Who proposed this? The solid sphere model of the atom

A

John Dalton

46
Q

Who proposed this? The raisin bun model

A

Joseph John Thomson

47
Q

Who proposed this? Nuclear model of an atom.

A

Ernest Rutherford

48
Q

Who proposed this? Planetary model of an atom

A

Neils Bohr

49
Q

Who proposed this? Bohr-Sommerfeld atomic model

A

Neils Bohr and Arnold Sommerfeld

50
Q

Who conducted the gold foil experiment?

A

Ernest Rutherford

51
Q

Neutrons and protons are collectively known as?

A

Nucleons

52
Q

Mass of an electron compared to a proton

A

1/1837 of the mass of the proton

53
Q

Ion with positive charge

A

Cation

54
Q

Ion with negative charge

A

Anion

55
Q

Number of protons in an element

A

Atomic Number

56
Q

Symbol for atomic number

A

Z

57
Q

The sum of the numbers of protons and neutrons in an atom

A

Mass number

58
Q

Symbol for Mass Number

A

A

59
Q

Atoms of the same element may have the same atomic number, but the atomic mass may differ. These atoms are called?

A

Isotopes

60
Q

An atom of a specific isotope is called?

A

Nuclide

61
Q

Mass number

A

Number of protons+ number of neutrons

62
Q

Number of neutron

A

Atomic Number- mass number

63
Q

Formulated the Uncertainty Principle

A

Werner Heisenberg

64
Q

State the uncertainty principle

A

It is impossible to determine both the momentum and the position of an electron at the same time accurately

65
Q

Proposed the quantum mechanical model of an atom

A

Erwin Schrodinger

66
Q

Lowest energy level or energy state of an electron

A

Ground state

67
Q

Highest energy state for an electron

A

Excited state

68
Q

The highest occupied energy level or electron shell

A

Valence shell

69
Q

Electrons occupying the valence shell

A

Valence electrons

70
Q

Obtained when the shell is completely filled with the assigned electrons

A

Closed shell

71
Q

A spherical cloud that becomes less dense as the distance from the nucleus increases. The electrons in this orbital possess lower energy because they are found close to the nucleus

A

S orbital

72
Q

It is a dumbbell-shaped cloud, having two lobes on opposite sides of the nucleus. The electrons here can never be found near the nucleus.

A

P orbital

73
Q

It is like a four leaf clover, an hour and a ring.

A

D orbital

74
Q

Are difficult to represent, and it is too complex to visualize them.

A

F orbital

75
Q

Used to describe an electron in an orbit or atomic orbital, the region in space with the greatest probability of finding the electron in an atom.

A

Quantum numbers

76
Q

Designates the energy level of each atomic orbital in which the electron moves. It also determines the average distance of the electron from the nucleus. It also describes the electron shell.

A

The principal quantum number (n)

77
Q

Also called angular momentum number or subsidary number, this one describes the way the electron moves around the nucleus. This describes the general shape of the orbital whether it is s, d, p, or f orbital and this tells the sub-level or sub-shell to which the electron belongs.

A

Azimuthal quantum numbers (l)

78
Q

Describes the spatial orientation of an electron in a space or magnetic field.

A

The magnetic quantum number (ml)

79
Q

Specifies the way the electron spins or rotates, either counterclockwise or clockwise, on its axis as it moves within the orbital.

A

The electron spin quantum number (ms)

80
Q

The arrow up in the electron spin quantum number signifies a __________ movement.

A

Counterclockwise

81
Q

The arrow down in the electron spin quantum number signifies a ___________ movement.

A

Clockwise movement

82
Q

The probable distribution of electrons around the nucleus among the orbitals is called?

A

Electron configuration

83
Q

Hund’s rule is also called?

A

Principle of minimum pairing and the principle of maximum multiplicity.

84
Q

If all the electrons in an atom are paired, the atom is?

A

Diamagnetic

85
Q

It is the atom that contains unpaired electrons that is drawn to a magnetic field.

A

Paramagnetism

86
Q

Maximum electrons in the 1st level?

A

2

87
Q

Maximum electrons in the second level?

A

8

88
Q

Maximum electrons in the 3rd level?

A

18

89
Q

Maximum electrons in the 4th level

A

32

90
Q

Maximum electrons in the 5th level

A

50

91
Q

Maximum electrons in the 6th level

A

72

92
Q

Pieces or energy are known as?

A

Quanta

93
Q

Chemicals symbols were invented by?

A

Jons Jacob Berzelius

94
Q

Arranged the 33 elements into four categories

A

Antoine Lavoisier

95
Q

Studied three elements and attempted to arrange the elements as triads

A

Johannes Wolfgang Dobereiner

96
Q

Had the idea to plot the elements in a spiral around the surface of the cylinder divided into 16 vertical sections according to the elements’ atomic masses.

A

Beguyer de Chancourtois

97
Q

Beguyer de Chancourtois’s device

A

Telluric helix

98
Q

Proposed the law of octaves

A

John Newlands

99
Q

Arranged the elements by their increasing atomic masses in a horizontal row

A

Dmitri Ivanovich Mendeleev

100
Q

Discovered the noble gases

A

William Ramsay

101
Q

Arranged the elements by their atomic numbers.

A

Henry Moseley

Science(Random) (4 decks)

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