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AP Chemistry > H Chemistry: Unit 3 > Flashcards

H Chemistry: Unit 3 Flashcards

1
Q

Democritus (400 B.C.)

A

-matter is composed of empty space through which atoms move
-atoms are solid, indestructible, and indivisible
-different properties of matter are due to different types of atoms
-changes in matter result from changes in the groupings of atoms
-discredited by Aristotle

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2
Q

John Dalton (1800)

A

-all matter is composed of atoms
-all atoms of a given element are identical
-atoms cannot be created or divided
-atoms combine in simple whole numbers to form compounds
-atoms are rearranged in chemical reactions
-atoms are divisible into subatomic particles
-atoms of the same element can have slightly different masses

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3
Q

atom

A

smallest particle of an element that retains all the properties of the element

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4
Q

Irving Langmuir (1881)

A

-established the size of an atom
-american scientist

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5
Q

size of an atom

A

1 billionth of a meter in diameter

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6
Q

Sir William Crookes (1820)

A

invented the cathode ray

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7
Q

cathode ray

A

glass tube hooked to a vacuum pump that is hooked up to two different charged electrodes

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8
Q

cathode

A

negative

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9
Q

anode

A

positive

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10
Q

J.J. Thomson (1890s)

A

-performed experiments with the cathode ray tube using magnets and found the negatively charged particles to be smaller than the atom
-credited for discovering electrons

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11
Q

plum pudding atomic model

A

negatively charged electrons are distributed throughout positively charged matter; sphere

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12
Q

Robert Milikan (1909)

A

-calculated the actual charge of the electron
-determined the mass of the electron

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13
Q

mass of the electron

A

9.1 x 10 ^-28 g

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14
Q

Ernest Rutherford (1911)

A

-gold foil experiment
-credited for discovering the nucleus of the atom and the proton
-nuclear model

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15
Q

gold foil experiment

A

where a narrow beam of positively charged alpha particles pass through a thin piece of gold foil and were reflected on a zinc sulfide screen

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16
Q

James Chadwick (1932)

A

discovered the neutron and that it has mass equal to that of a proton

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17
Q

Niels Bohr (1920-1940)

A

-improved Rutherford’s model by placing electrons at specific energy levels
-Bohr’s model

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18
Q

atomic number

A

indicates the number of protons

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19
Q

proton

A

positively charged subatomic particle located in the nucleus
-identifies the atom
-not gained or lost naturally in the lab

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20
Q

electron

A

negatively charged subatomic particle that orbits the nucleus
-determines reactivity
-number is the same as number of protons if atom is neutral

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21
Q

ion

A

charged atom from the gain or loss of electrons

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22
Q

anion

A

negatively charged ion from the gain of electrons

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23
Q

cation

A

positively charged ion from the loss of electrons

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24
Q

atomic mass

A

indicates the number of protons and neutrons together
-units are amu

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25
Q

mass of a proton/neutron

A

1 amu

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26
Q

neutron

A

neutrally charged subatomic particle in the nucleus of an atom
-calculated by taking the atomic mass and subtracting the atomic number

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27
Q

why is the atomic mass not a whole number

A

1) the mass of the proton and neutron in different elements differ slightly
2) the atomic mass is an average of all the isotopes of the element and their frequency

28
Q

isotope

A

atoms of the same element with different masses because they have different numbers of neutrons

29
Q

amu

A

-atomic mass unit
-1/12 of C-12

30
Q

electromagnetic radiation

A

all forms of energy that travels in waves

31
Q

wave length

A

distance between two identical points on a wave; measured in meters or nanometeres

32
Q

frequency

A

number of waves that pass through a given point in 1 second; measured in inverse seconds or s^-1 or Hertz(Hz)

33
Q

amplitude

A

energy in wave initiation

34
Q

all electromagnetic radiation travels at

A

the same speed; c= 3.0 x 10^8 m/s

35
Q

wave length is inversely related to

A

frequency, as wave length increases, frequency decreases

36
Q

electromagnetic spectrum

A

list of all types of electromagnetic radiation

37
Q

electromagnetic spectrum in order

A

radiowaves, microwaves, infrared radiation, visible light, ultraviolet, x-rays, gamma rays

38
Q

Max Planck

A

experimented with heating objects and cooling them, he noticed that heat/energy was absorbed and released in “chunks”

39
Q

quantum

A

minimum amount of energy that can be absorbed or released by an atom

40
Q

photon

A

packet of energy that carries a quantum

41
Q

energy does not exist

A

between the units

42
Q

energy equation

A

E=hv (Planck’s constant)(frequency)

43
Q

Planck’s Constant

A

6.626 x 10 ^-34 Js

44
Q

atomic emission spectrum

A

unique band of colors emitted from an element when heated

45
Q

Albert Einstein

A

propose that light is both a particle and a wave

46
Q

photoelectric effect

A

light at a certain frequency when shined upon a specific metal will emit photoelectrons(no matter the duration or intensity)

47
Q

Heinsburg Uncertainty Principle

A

you cannot know both the velocity and the location of an electron at the same time

48
Q

quantum numbers

A

used to determine the location of an electron in an atom

49
Q

1 principle quantum number

A

-primary energy level
-positive number that corresponds to the period on the periodic table
-higher the n, the higher the energy(usually)
-not a distance

50
Q

2 angular momentum quantum number(l)(energy sub level)

A

-shows the shape of the orbital

51
Q

orbital

A

region where there is a strong likelihood of finding an electron

52
Q

s orbital

A

spherical

53
Q

p orbital

A

dumbell

54
Q

d orbital

A

shape varies

55
Q

f orbital

A

shape varies

56
Q

3 magnetic quantum number(Ml)

A

reveals the spacial orientation of the orbital

57
Q

4 spin quantum number(Ms)

A

reveals the spin of the electron

58
Q

pauli exclusion principle

A
  1. No two electrons can have the same four quantum numbers
  2. No more than two electrons in an orbital
59
Q

orbital diagram

A

illustration of electron configuration
- arrow represents an electron

60
Q

orbital diagram- s orbital

A

1 box

61
Q

orbital diagram- p orbital

A

3 boxes

62
Q

orbital diagram- d orbital

A

5 boxes

63
Q

orbital diagram- f orbital

A

7 boxes

64
Q

Hund’s rule

A

electrons will occupy an empty orbital of the same energy level before pairing up to avoid repulsion

65
Q

afbau diagram

A

orbital filing diagram

66
Q

valence electron

A

electron in the highest energy that are directly involved in bonding

67
Q

lewis dot diagram

A

illustration of valence electrons

AP Chemistry (16 decks)

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