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intro to Chem > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

The total mass of a substance does not change during a chemical reaction

A

Law of mass conservation

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2
Q

A given compound always has the same composition / same amount of ratio of elements

A

Constant composition

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3
Q

When two elements react to form more than one compound

A

Law of multiple proportions

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4
Q

Hydrogen and oxygen can combine to create both H2O (water) and hydrogen peroxide (h2o2) is an example of

A

Law of multiple proportions example

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5
Q
  1. Elements are made up of atoms
  2. An elements atoms are identical
  3. Atoms of an element will differ from other elements.
  4. Atoms of one element combined with atoms of another element create a compound
  5. Atoms are indivisible in a chemical process
A

Daltons atomic theory

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6
Q

Used to study charge particles

A

Cathode ray tube

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7
Q

Used to find out the charge of an electron

A

Milligan’s oil drop experiment

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8
Q

The main premise of the Millikan oil drop experiment

A

The oil droplets with the higher amount of positively charged electrons would sink faster to the bottom

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9
Q

The smallest difference in speeds of oil droplets in Millikans experiment happened

A

The difference of 1 electron

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10
Q

The 3 key characteristics of an electron

A
  1. Negative charged particles
  2. Very light compared to an atom
  3. They move rapidly within the atom
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11
Q

The mass of an electron

A

1/1836th the mass of a Hydrogen atom

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12
Q

The mass of an atom is not due to

A

Electrons

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13
Q

The atom

A

A cloud of positive charge with very small particles of negative charge embedded in it

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14
Q

An electron

A

Negative charge

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15
Q

Alpha particles are

A

Small positively charged particles

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16
Q

The alpha particles that were reflected in the gold experiment

A

Hit the nucleus.

*what happened to the the alpha particles when it hit the nucleus

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17
Q

The nucleus has a __ charge?

A

Positive charge

  • a positive charge in the nucleus is what
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18
Q

The center of a atom

A

The nucleus

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19
Q

Majority of the volume of an atom consists of

A

Electrons

*electrons are the majority of what

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20
Q

The size of a nucleus

A

Is very small

*what is very small in a atom?

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21
Q

What is a common expression said about atoms?

A

That they are empty space

*”made up of empty space” is a common answer to what

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22
Q

Uncharged particles

A

Neutrons

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23
Q

Neutrons have a mass of __ and a charge of __

*neutrons

A

1 and zero.

  • what has a mass of one and a charge of zero
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24
Q

What is mass?

*mass

A

The quantity of matter in an object

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25
The structure of the nucleus consists of *nucleus
Protons and neutrons *protons and neutrons make up the structure of
26
2000 times the mass of a neutron
Proton (size)
27
Charge of a proton
+1
28
Charge 0
Neutron (charge)
29
A neutral atom
of protons = # of electrons
30
This particle defines an element *it defines it
A proton *a proton has what relationship with an element
31
Visualize this in your head - where is the mass number located?
Top left | Skip
32
The mass number equals
of p + # of n
33
Visualize this in your head - The atomic number is located?
Bottom left
34
The atomic number equals
#of protons OR # of e for neutral atoms
35
Electrons are
Negative charged particles in an atom
36
Isotopes
Atoms with the same number of protons but different number of neutrons
37
To determine the isotopes
Atomic numbers must be the same
38
The nucleus is composed of
Positively charged protons and uncharged neutrons
39
The nucleus is surrounded by
Negatively charged electrons
40
The mass of an atom is
Derived mainly from the nucleus
41
Why is the majority of the mass inside of the nucleus
Because protons and neutrons are much heavier than electrons
42
Go from heaviest to lightest with e,p, and n
Neutrons heaviest, then protons, then electrons which are lightest *skip
43
The atomic number
The number of protons in the nucleus is
44
Defining trait in an element
Number of protons in the nucleus *skip
45
Atomic number =
Number of protons *skip
46
All atoms have the same __ but can have a different ___
Atomic number; mass number
47
Isotopes
Atoms with the same atomic number (protons) but not the same mass number (different neutrons)
48
If you are given the atomic mass and the atomic number how do you find the amount of neutrons
Mass minus the atomic number
49
Radiation with no electric charge
Gamma rays
50
Radiation with a negative charge
Beta particle
51
Radiation with a positive charge
Alpha particles
52
Weight of alpha,beta, gamma particles
1. Heavy weight 2. medium weight 3. Light weight
53
Penetrating abilities of particles
Alpha particles can be stopped by thick paper Beta particles by aluminum foil Gamma rays by a lead wall
54
Gamma rays and x rays are forms of
Electromagnetic radiation
55
Gamma rays in comparison to x rays
Shorter wave length and higher energy
56
Strong nuclear force
Protons should repel each other in the nucleus. This keeps it together
57
Electrostatic force
repulsive force between two electrically charged objects
58
Where do alpha particles come from
When the nucleus becomes to big it becomes unstable and some particles will fall apart
59
Alpha particle has an elemental nucleus of
Helium *skip
60
Alpha particles - protons and neutrons
2 protons and 2 neutrons
61
Alpha particle is related to which element?
Helium
62
Alpha decay means
Minus the mass (4) and the atomic number (2) from the element
63
A beta particle can also be known as a
Electron *skip
64
Instead of an atomic number, what would you put for a beta particle?
-1
65
Mass of a beta particle
0
66
What happens to the atomic number in beta decay?
It increases *skip
67
beta decay increase the atomic number
Neutrons become protons
68
mass and atomic number for protons
1 and 1
69
Mass spectrometer
Used to measure isotopes
70
Average atomic number
Is the average of all the isotopes of an element
71
The simple version of isotopes
Different versions of an element or a type of atom
72
Isotopes protons and neutrons
Have the same protons but different neutrons
73
Calculation of the average atomic mass of an element
Atomic mass x percentage/100 Do that to all them then add all together
74
ions
atoms or groups of atoms with an electrical charge
75
two types of atoms
cations | anions
76
cations
positively charged ions result from losing an electron
77
anions
negative charged ions resulting from a gain of an electron
78
neutral atom
protons = electrons
79
formation of ions
gaining or losing electrons
80
removing or adding protons
change in element
81
ions do or do not change the element
do not *skip
82
the amount of protons
atomic number
83
the amount of neutrons
atomic number minus the mass number
84
the amount of electrons
its the same amount as protons (atomic number) but look if it has an electrical charge
85
element with a negative in the top right, what does that do to the number of electrons?
adds one electron *skip
86
a positive charge on an element tells you what
how many electrons you need to subtract
87
a negative charge on an element tells you what
how many electrons you need to add
88
posititve charges or cations are metals t/f
true *skip
89
how are the elements organized on the periodic table in relation to their charge
the elements with the same charge are in the same column *skip
90
noble gases in relation to their ions
this column does not contain ions on the periodic table
91
compound
formed when two or more elements combine together in a fixed ratio
92
3 types of chemical formulas
molecular, structural, emperical
93
molecular formula
shows the actual composition of a molecule
94
structural formula
shows the actual composition of a molecule and how the atoms are connected
95
emperical formula
shows the simplest whole number ratio between the atoms in a compound
96
stable/unstable: noble gases
very stable
97
stable/unstable: alkali metals
unstable
98
3 Properties of non metals
Not shiny, not malleable, poor conductors of heat and electricity
99
Period and group meaning
Laterally, up and down periodic table
100
Allotropes
Different forms of the same element in the same state

intro to Chem (11 decks)

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