CH 1A Flashcards

(65 cards)

1
Q

describe two central ideas of chemistry

A
  1. Matter is made of particles
  2. the structure of these particles determines the properties of matter
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2
Q

Differences in the properties of these metal arise from what differences?

A

differences in the structure of their particles

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3
Q

What are the three classifications of solid matter?

A
  1. energy too low to overcome forces
  2. tightly packed
  3. fixed in place
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4
Q

What are the three classifications of liquid matter?

A
  1. energy sufficient to overcome some forces
  2. closely packed
  3. can move
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5
Q

What are the three classifications of gaseous matter?

A
  1. energy sufficient to overcome some forces
  2. closely packed
  3. can move
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6
Q

what are the three classifications of gaseous matter?

A
  1. energy sufficient to overcome all forces
  2. widely spaced
  3. freely move
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7
Q

What particles make up matter?

A

atoms

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8
Q

what are atoms?

A

smallest basic particle

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9
Q

How many different types of particles are there?

A

118 (91 form naturally)

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10
Q

what are the three fundamental particles of matter?

A
  1. individual atoms
  2. molecules
  3. repeating unit of atoms
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11
Q

give an example of individual atoms?

A

Helium (He)

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12
Q

what is a molecule?

A

atoms bonded together in specific geometrical arrangements

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13
Q

give an example of a molecule

A

Ozone O3, Hydrogen Peroxide (H2O2)

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14
Q

what are repeating units of atoms

A

repeating units of atoms are the consistent, repeating arrangement of atoms in a crystalline or structured form.

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15
Q

give an example of repeating units of atoms

A

Sodium chloride (NaCl

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16
Q

what is the difference between repeating units of atoms and molecules?

A

Repeating units of atoms refer to the pattern or arrangement of atoms in a material, particularly in solid forms.
Repeating units of molecules refer to the individual molecular units or monomers that repeat to form larger molecules like polymers.

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17
Q

What is a pure substance?

A

a substance that contains one type of particle

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18
Q

What are two types of pure substances?

A

elements and compounds

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19
Q

What is an element?

A

a pure substance that can’t chemically break down into simpler substances

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20
Q

What is a compound?

A

A pure substance composed of two or more elements bonded together in fixed definite proportions. (more than one type of atom bonded together)

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21
Q

Can a compound be broken down?

A

Yes, compounds can be broken down into elements by a chemical reaction

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22
Q

Give an example of compounds

A

Sodium chloride (NaCl)

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23
Q

what is matter that isn’t made up of one particle?

A

Mixtures

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24
Q

what are mixtures?

A

two or more pure substances blended together in proportions that can vary

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25
what are two types of mixtures?
heterogeneous and homogeneous mixtures
26
what are heterogeneous mixtures
mixings that are NOT uniform such that the composition isn't uniform.
27
give an example of a heterogeneous mixture
sand, cereal in milk, oil and water,
28
what are homogeneous mixtures
mixings that ARE uniform such that the composition is the same throughout
29
what are examples of homogenous mixtures
Vega's drink, air, wine, coffee
30
How do we know that matter is made of particles?
experimental evidence
31
How do we know that matter is made of particles?
Experimental evidence
32
Law of conservation of mass
mass of reactants equals the mass of the products for a chemical reaction
33
law of definite proportions
In any given chemical compound, the elements are always combined in the same proportion by mass.
34
law of multiple proportions
When two elements form more than one compound, the different masses of one element that combine with a fixed mass of the other element are in a ratio of small whole numbers.
35
Lavoisier discovered . . .
the law of conservation of mass
36
how did Lavoisier discover the law of conservation of mass
by inventing balances, allowing him to weigh the reactions before and afterwards. Shows that the mass was conserved
37
Does the mass of reactants = the mass of products
Yes
38
give an example of mass of reactant = mass of products
2HgO--> 2Hg + O2
39
what are the four points of Dalton's atomic theory?
1. each element is composed of tiny indestructible particles called atoms 2. all atoms of a given element have the same mass and properties; these distinguish them from other elements. 3. Atoms combine in simple, whole-number ratios to from compounds 4. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way they are bound together with other atoms.
40
Key characteristics of the scientific method are
observations formulation of hypotheses experimentation formulation of laws and theories
41
A hypothesis is a
interpretation or explanation of the observations
42
A scientific law
is a brief statement that summarizes past observations and predicts future ones. describes patterns
43
Name a scientific law
law of conservation of mass
44
A scientific theory is
formed from a well-established hypothesis or set of hypotheses. A theory tries to explain why a natural phenomenon happens. (greatest degree of certainty in science)
45
name a scientific theory
dalton's atomic theory
46
in science, a theory is
what scientist are MOST CERTAIN about
47
Atoms are made up of what three subatomic particles
protons, neutrons, and electrons
48
What is the mass of a proton
1.67262 x 10^-27
49
What is the mass of a neutron
1.67262 x 10^-27
50
what is the mass of a electron
0.00091x10^-27
51
A proton's charge is
1+
52
A neutron's charge is
0
53
An electron's charge is
-1
54
How are atoms arranged?
An atom is spherical, composed of a positively charged central nucleus surrounded by one or more negatively charged electrons
55
atomic nucleus consists of
protons and neutrons
56
Describe Rutherford's gold foil experiment
He took a gold foil and shot alpha particles through the foil. The alpha particles, upon shooting through, ended up passing through with little deflection. But a small fraction was very strongly deflected, due to encountering something very massive. Suggesting that there was a very small and concentrated volume of protons and neutrons.
57
What was the predicted result of the rutherford's experiment
plum-pudding mode, where the particles are distributed evenly throughout
58
What was the actual result of rutherford's experiment
nuclear model, where the protons and neutrons are centered in a small area
59
What was the conclusion of rutherford's experiment
most of the atom is empty space with its mass largely concentrated in a tiny central core (nucleus)
60
atomic number is
the number of protons in an atom
61
mass number
the sum of the number of protons and neutrons in an atom
62
ion
an atom with a net charge due to loss or gain of electrons
63
isotopes
atoms with the same number of protons but different numbers of neutrons
64
mass number is located
on the top left of the chemical symbol
65
atomic number is located
on the bottom left of the chemical number