Chpt 5 Flashcards

(41 cards)

1
Q

Daltons Model (disproven)

A
  • elements made indivisible, indestructible particles called atoms
  • all atoms of element are identical & have same properties
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2
Q

Daltons Model (true)

A
  • atoms of different elements combine forming compounds
  • compounds contain atoms in small whole number ratios
  • atoms can combine in more than than one way to form different compounds
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3
Q

Thompsons Model

A

dense positive charge w/ negative charge electrons interspersed

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4
Q

Rutherfords Gold foil experiment

A

alpha particles were directed at a thin sheet. most passed few deflected -> atomic nucleus

a) if plum pudding model correct, alpha particles would pass without deflection
b) since small number deflected -> idea most of mass and all +charge of atom concentrated in space smaller than nucleus size

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5
Q

atomic number

A

(Z) number of protons (also # electrons if a neutral atom)

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6
Q

Mass number

A

(A) total # of protons & neutrons in nucleus of atom

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7
Q

similarities b/t protons electrons

A

protons and electrons same -> atom neutral

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8
Q

isotopes

A
  • atoms of same element with different number of neutrons

- have same atomic number

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9
Q

amu

A

atomic mass number

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10
Q

electromagnetic radiation

A

type of energy travels thru space at 3.0 x 10^8 m/s exhibits wave and particle like behavior.
e.g. light

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11
Q

wavelength (lamba)

A

distance between adjacent wave crests

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12
Q

frequency (v)

A

of cycles or crests that pass thru stationary point in one sec.

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13
Q

white light

A

continuous spectrum

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14
Q

light

A

visible radiant energy

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15
Q

visible spectrum

A

region of light spectrum our eyes can see

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16
Q

radiant energy spectrum (EM spectrum)

A

continuous spectrum of visible and invisible light that ranges from short to long lamba.

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17
Q

wave length *

A
  • increases to the left

- longer wavelength = lower frequency

18
Q

wavelength and frequency

A

inversely related

19
Q

wavelength and energy

A

inversely related

20
Q

frequency and energy

A

directly related

21
Q

x rays

A

ionizing radiation

22
Q

ultraviolet (UV) and infrared (IR) light

A

invisible to human eye

23
Q

microwaves

A

absorbed by water molecules and used to heat water containing substances

24
Q

ROYGBIV

A

red. orange. yellow. green. blue. indigo. violet.

25
photon
packet of light energy
26
quantum concept
energy is composed of discrete units (its quantized)
27
energy level
electrons travel in fixed energy orbits
28
bohr atom
electrons exits in specific distances from nucleus and occupy orbits of discrete energy levels
29
emission light spectrum
associated with emission of electromagnetic radiation by elements or compounds; collection of narrow bands of light energy
30
quantum numbers
energy of each bohr orbit has specific numbers (n=1,2,3...)
31
quantized
fixed
32
ground state
lowest energy state
33
excited state
when an electron is in a higher energy orbital
34
subshell
(energy sublevel) s (sphere), p(dumbbell), d (clover leaf), and f (no specific shape)
35
8A
noble gases
36
electron configuration
shows occupation of orbitals by electrons for particular atoms that is
37
subatomic particles
positive (+) negative (-) neutron
38
2 types of atomic notation
^3H & H-3
39
calculating protons neutrons and electrons
- neutrons = mass number - atomic number - protons = atomic number - identify element by # of protons
40
bohr model of atom
- energy levels (n=1,2,3...) - energy levels correspond to periodic table - energy levels are aka principal quantum numbers energy levels get closer the further away are from nucleus
41
electromagnetic radiation lab
- continuous spectrum (white light) produces rainbow - color of each discharge tube - 1 electron relaxing = 1 photon emitted