Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

atom

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Irving Langmuir (1881)

A

-established the size of an atom
-american scientist

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

size of an atom

A

1 billionth of a meter in diameter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Sir William Crookes (1820)

A

invented the cathode ray

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

cathode ray

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

cathode

A

negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

anode

A

positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

plum pudding atomic model

A

negatively charged electrons are distributed throughout positively charged matter; sphere

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Robert Milikan (1909)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

mass of the electron

A

9.1 x 10 ^-28 g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Ernest Rutherford (1911)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

James Chadwick (1932)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Niels Bohr (1920-1940)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

atomic number

A

indicates the number of protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

proton

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

ion

A

charged atom from the gain or loss of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

anion

A

negatively charged ion from the gain of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

cation

A

positively charged ion from the loss of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

atomic mass

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
mass of a proton/neutron
1 amu
26
neutron
neutrally charged subatomic particle in the nucleus of an atom -calculated by taking the atomic mass and subtracting the atomic number
27
why is the atomic mass not a whole number
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
isotope
atoms of the same element with different masses because they have different numbers of neutrons
29
amu
-atomic mass unit -1/12 of C-12
30
electromagnetic radiation
all forms of energy that travels in waves
31
wave length
distance between two identical points on a wave; measured in meters or nanometeres
32
frequency
number of waves that pass through a given point in 1 second; measured in inverse seconds or s^-1 or Hertz(Hz)
33
amplitude
energy in wave initiation
34
all electromagnetic radiation travels at
the same speed; c= 3.0 x 10^8 m/s
35
wave length is inversely related to
frequency, as wave length increases, frequency decreases
36
electromagnetic spectrum
list of all types of electromagnetic radiation
37
electromagnetic spectrum in order
radiowaves, microwaves, infrared radiation, visible light, ultraviolet, x-rays, gamma rays
38
Max Planck
experimented with heating objects and cooling them, he noticed that heat/energy was absorbed and released in "chunks"
39
quantum
minimum amount of energy that can be absorbed or released by an atom
40
photon
packet of energy that carries a quantum
41
energy does not exist
between the units
42
energy equation
E=hv (Planck's constant)(frequency)
43
Planck's Constant
6.626 x 10 ^-34 Js
44
atomic emission spectrum
unique band of colors emitted from an element when heated
45
Albert Einstein
propose that light is both a particle and a wave
46
photoelectric effect
light at a certain frequency when shined upon a specific metal will emit photoelectrons(no matter the duration or intensity)
47
Heinsburg Uncertainty Principle
you cannot know both the velocity and the location of an electron at the same time
48
quantum numbers
used to determine the location of an electron in an atom
49
#1 principle quantum number
-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
#2 angular momentum quantum number(l)(energy sub level)
-shows the shape of the orbital
51
orbital
region where there is a strong likelihood of finding an electron
52
s orbital
spherical
53
p orbital
dumbell
54
d orbital
shape varies
55
f orbital
shape varies
56
#3 magnetic quantum number(Ml)
reveals the spacial orientation of the orbital
57
#4 spin quantum number(Ms)
reveals the spin of the electron
58
pauli exclusion principle
1. No two electrons can have the same four quantum numbers 2. No more than two electrons in an orbital
59
orbital diagram
illustration of electron configuration - arrow represents an electron
60
orbital diagram- s orbital
1 box
61
orbital diagram- p orbital
3 boxes
62
orbital diagram- d orbital
5 boxes
63
orbital diagram- f orbital
7 boxes
64
Hund's rule
electrons will occupy an empty orbital of the same energy level before pairing up to avoid repulsion
65
afbau diagram
orbital filing diagram
66
valence electron
electron in the highest energy that are directly involved in bonding
67
lewis dot diagram
illustration of valence electrons

AP Chemistry (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions