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CHEM111 > MIDTERM (chp3-4) > Flashcards

MIDTERM (chp3-4) Flashcards

1
Q

Atom

A

Smallest particle of an element that still has the properties of the element

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2
Q

Molecule

A

A group of two or more atoms that function as a unit because the atoms are tightly bounded together

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3
Q

Dmitri Mendeleev

A

Organized known elements into a table based on atomic mass, and similar properties into columns

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4
Q

Rules/ facts of atoms (5)

A
  • 118 types of atoms
  • All atoms of given element are similar to one another
  • Atoms of one element combine with atoms of other elements to form compounds
  • A compound always has the same relative numbers and types of atoms
  • During chemical reactions, changes only occur in the way atoms are grouped together
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5
Q

Group (3):

A
  • Verticle column
  • Contains elements with similar chemical properties
  • Column numbered 1-18
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6
Q

Period (2):

A
  • Horizontal row of elements left to right
  • Elements in the same row are not related chemically
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7
Q

Metals

A

Usually solid at room temperature btu can be molded into different shapes, and conduct heat/electricity

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8
Q

Nonmetals

A

Absence of lustre, thermal and electrical conductivity, malleability

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9
Q

Metalloids

A

Semiconductors. Can conduct electricity, but not as efficiently as metals

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10
Q

1890s J.J Thompson’s Experiment

A

Found that electrical charges were created when electrons are transferred to or removed from an object

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11
Q

1911 Ernest Rutherford

A

Stated that atoms are neutral therefore there must be a positive component

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12
Q

Ernest Rutherford experiment

A

Directed positive alpha particles toward a thin metal foil and found that most alpha particles passed through but some deflected. He concluded that there must be a large centre of concentrated positive charge in atom

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13
Q

Plum pudding model

A

Negatively charged electrons embedded with a positively charged “soup”

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14
Q

Nucleus

A

Dense centre of positive charge containing + charged particles, protons, neutral particles, neurons

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15
Q

Protons

A

Particles of positive charge in contained nucleus (number of protons must be equal to the number of electrons)

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16
Q

Neutrons

A

Neutral particles in nuclei

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17
Q

Electrons

A

Particles of negative charged fill space around nucleus

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18
Q

Why does chemistry of an atom arise from its electrons?

A

Because electrons are outside the nucleus in the outer regions of the atom and they interact when atoms come closer. Thus atoms can gain or lose electrons during chemical reactions

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19
Q

Atomic number

A

Characteristic of element, equal to number of protons in nucleus and electrons in the neutral atom

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20
Q

Mass number

A

Equal to the number of protons and the number of neutrons in the nucleus of the atom

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21
Q

Isotopes

A

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

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22
Q

Isobars

A

Atoms that have the same mass number but different atomic number so they are different elements

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23
Q

Ions

A

Formed when electrons are added to, or removed from a neutral species

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24
Q

Cation

A

A positively charged ion resulting from removing 1 or more electrons from a neutral species

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25
Q

Anion

A

Negatively charged ion that result from a neutral species gaining one or more electron

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26
Q

Simple ions

A

Charged species containing only one atom

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27
Q

Polyatomic ion

A

Charged species containing a group of atoms held together by strong bonds

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28
Q

Solar system model

A

Describes atoms as consisting of a nucleus with a number of electrons in orbits around that nucleus

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29
Q

Quantum Mechanics Model

A

Arises from a mathematical description of the behavior of an electron in a hydrogen atom. Electron does not travel in a circular orbit

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30
Q

Law of conservation of mass

A

States that in chemical reactions, matter is neither created nor destroyed created by Antoine Lavoisier

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31
Q

Atomic theory by John Dalton

A
  • Elements are made of tiny indivisible particles called atoms
  • Atoms of each element are unique
  • Atoms can join together in whole number ratios to form compounds
  • Atoms are unchanged in chemical reactions
32
Q

Scanning tunneling microscopy

A

Technique from early 90s that was used to visualize atoms on a mental surface and move them to form letters

33
Q

X-ray crystallography

A

Used to determine the atomic and molecular structure of a crystal, in which the crystalline structure causes a beam of incident x-rays

34
Q

Main group elements

A

Blocks of elements on the left and right side of periodic table (1A-8A)

35
Q

Transition elements

A

Elements in the middle of table. They are harder and less reactive than metals 1-2

36
Q

Inner transition elements

A

Bottom of the periodic table (the 2 additional rows)

37
Q

Lanthanide series

A

Inner transition elements that are metals. Contains heavier, naturally occurring metals called the rare earth metals

38
Q

Actinide series

A

Second row of the inner transition elements. The first few elements in this series (up to uranium) are naturally occurring. The elements that occur after uranium are mostly human-made

39
Q

Alkali metals

A

Far left of periodic table. Soft metals that react violently with air or moisture (eg. Lithium, sodium, potassium)

40
Q

Alkaline earth metals

A

Right of the alkali metals. Elements are reactive but less violently than alkali metals. Will react slowly with water but burn brightly when combined with oxygen (eg. Magnesium, calcium)

41
Q

Halogens

A

Elements in column 7A. Exist as diatomic (two-atom) molecules and react quickly with metals and nonmetals to form different compounds (eg. Bleach, Teflon, fire retardants)

42
Q

Noble gases

A

Elements in column 8A. Stable and generally do not react with other elements to form compounds. All gasses at room temperature (eg. Helium, neon)

43
Q

Alessandro Volta (2):

A
  • Built the first battery (electrochemical cell)
  • Placing alternate plates of zinc and copper on either sides of pieces of cardboard soaked in sulfuric acid
44
Q

Electron cloud

A

Space around nucleus

45
Q

Wavelength

A

The distance from a point on one wave to the same point on the next wave

46
Q

Frequency

A

Number of waves (cycles) per second that pass a given point in space

47
Q

Speed

A

Product of the wavelength and its frequency

48
Q

Planck’s constant

A

Universal constant that relates the energy of a photon to its frequency (6.626 x 10^-34)

49
Q

Subshells of electron

A

s p d f

50
Q

Aufbau building up principle

A

Electrons go into available orbitals one at a time, filling each orbital of lowest energy before going to the next energy level

51
Q

Hunds rule (Pauli exclusion)

A

No two electrons in a atom can have an identical set of four quantum numbers.

52
Q

Paramagnetic

A

Atoms, ions, or compounds whose electron arrangement result in one or more unpaired electrons. Paramagnetic materials are attracted into an external magnetic field

53
Q

Diamagnetic

A

Atoms, ions, or compounds whose electron arrangement results in all electrons paired in orbitals. They are slightly repelled by an external magnetic field

54
Q

Ground state electron configuration

A

The electrons are in the orbitals of lowest possible energy following the Aufbau principle and Hund’s rule (normal/resting state of an atom or ion)

55
Q

Excited state

A

Electrons can absorb energy and move into a higher energy orbital

56
Q

Distinguishing electron

A

the last electron that is added when you are building up the electron configuration of an atom

57
Q

Valence electrons

A

All electrons in the outermost electron shell (highest n level)

58
Q

Core electrons

A

All electrons that are not classified as valence electrons

59
Q

Alkali metal valence shell configuration

A

ns^1

60
Q

Alkaline earth metal valance shell configuration

A

ns^2

61
Q

Halogen valence shell configuration

A

ns^2np^5

62
Q

Noble gas valence shell configuration

A

ns^2np^5

63
Q

Electromagnetic radiation

A

Form of energy that travels in waves that are produced when charged particles move or vibrate relative to each other

64
Q

Electromagnetic spectrum

A

Range of electromagnetic energy from low energy waves (TV, radio waves) to very high waves (x-rays, gamma rays)

65
Q

Hertz

A

Frequency of one wave cycle per second (Hz) (1/s = 1s^-1 = 1Hz)

66
Q

How are wavelength and frequency related

A

if wavelength decreases, frequency increases & vice versa

67
Q

Flame test

A

Wire dipped in solution that contains metal ions. The ions of each element give off a characteristic color when heated (eg. Wire with calcium = orange, wire with copper = green). this is because different metals have a different patterns of spectral colours. Flame collars produced from movement of electrons

68
Q

Why does the sun give off light

A

The Sun is powered by a type of reaction called nuclear fusion, which releases an incredible amount of energy. This energy continually excites electrons (and other charged particles), which release this energy as electromagnetic radiation. The Sun radiates electromagnetic energy across the spectrum, not just visible light

69
Q

Why does a fire give off light

A

When a substance like wood burns, the carbon and hydrogen in the substance react with oxygen in the air. This reaction releases heat energy as well as gaseous products such as carbon dioxide and water vapor. The electrons within these compounds are excited to higher levels. As these gaseous products exit the reaction, their electrons release this energy as visible light that we see as flames

70
Q

Do you give off light

A

People don’t give off visible light; however, as your body produces heat, you release this energy in the form of infrared radiation. Specialized cameras can convert infrared energy into visible images, making it possible to “see” someone in the dark

71
Q

Fluorescence

A

Ability of certain chemicals to give off visible light after absorbing radiation which is not normally visible, such as ultraviolet light

72
Q

s sublevel

A

Simplest of the sublevels with only one orbital shaped like a sphere

73
Q

p sublevel

A

Contains three different orbitals. Each orbital has a shape similar to an infinity symbol

74
Q

d sublevel

A

Contains 4 orbitals and can hold a maximum of 10 electrons

75
Q

f sublevel

A

Contains 7 orbitals and can hold a maximum of 14 electrons

CHEM111 (6 decks)

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