Chapter 1 Flashcards

(67 cards)

1
Q

atoms or molecules have a lot of space between them. They are free to move relative to one another, making it compressible.

A

Gas

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2
Q

atoms or molecules pack about as closely as they do in solid matter, but they are free to move relative to each other.They have fixed volume but not a fixed shape.
Their ability to flow makes them assume the shape of their container.

A

Liquid

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3
Q

Atoms or molecules pack closely to each other in fixed locations. Although the atoms and molecules vibrate, they do not move around or past each other. Consequently, they have a fixed volume and rigid shape.

A

Solid

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4
Q

Matter can be classified according to

A
  1. It’s state
  2. It’s composition
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5
Q

Basic submicroscopic particles that constitute the fundamental building blocks of ordinary matter

A

Atoms

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6
Q

Substances formed when two or more atoms come together (bond) in specific geometric arrangements

A

Molecules

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7
Q

anything that has mass and occupies space

A

Matter

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8
Q

the discipline that seeks to understand matter and its properties.

A

Chemistry

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9
Q

If a substance is a pure substance, it can be classified as either an ____ or a ________.

A

Element;compound

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10
Q

made up of only one component, and its composition is invariant.

A

Pure substance

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11
Q

A substance composed of two or more components in proportions that can vary from one sample to another.

A

Mixture

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12
Q

a substance that cannot be chemically broken down into simpler substances.

A

Element

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13
Q

substance composed of two or more elements in fixed definite proportions.

A

Compound

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14
Q

a process for understanding nature by observing nature and its behavior through experimentation.

A

Scientific method

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15
Q

one made of multiple substances, but it appears to be one substance. All portions of a sample have the same composition and properties (like sweetened tea).

A

Homogeneous mixture

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16
Q

one in which the composition varies from one region of the mixture to another. Made of multiple substances, whose presence can be seen (e.g., a salt and sand mixture)

A

Heterogeneous mixture

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17
Q

They are also known as data.They are the descriptions about the characteristics or behavior of nature.

A

Observations

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18
Q

a tentative interpretation or explanation of the observations.

A

Hypothesis

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19
Q

A brief statement that summarizes past observations and predicts future ones

A

Scientific law

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20
Q

Law that states, “in a chemical reaction, matter is neither created nor destroyed.” is known as

A

Law of conservation of mass

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21
Q

A well-established hypothesis or set of hypotheses form the basis for a scientific ____

A

Theory

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22
Q

Which statement best explains the difference between a law and a theory?

(a) A law is truth whereas a theory is mere speculation.
(b) A law summarizes a series of related observations, while a theory gives the underlying reasons for them.
(c) A theory describes what nature does; a law explains why nature does it.

A

(b) A law summarizes a series of related observations, while a theory gives the underlying reasons for them.

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23
Q

______ and _____ were the first to propose that matter was composed of small, indestructible particle

A

Leucippus;Democritus

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24
Q

________wrote, “Nothing exists except atoms and empty space; everything else is opinion.”
He proposed that atoms existed in different shapes and sizes and moved randomly through empty space

A

Democritus

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25
______ and ______ did not embrace the atomic ideas of Leucippus and Democritus. –They held that matter had no smallest parts. –They proposed that different substances were composed of various proportions of fire, air, earth, and water.
Plato;aristotle
26
offered convincing evidence that supported the early atomic ideas of Leucippus and Democritus. Also known as Daltons atomic theory of matter
John Dalton
27
_________ explained the laws as follows: 1.Each element is composed of tiny, indestructible particles called atoms. 2.All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements. 3.Atoms combine in simple, whole-number ratios to form compounds. 4.Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms change only the way that they are bound together with other atoms.
Daltons atomic theory
28
All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements.
Law of definite proportions
29
The law of definite proportions was summarized by in 1797 by a French chemist named
Joseph Proust
30
When did John Dalton publish his law of multiple proportions
1804
31
Which law states, “When two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers.”
Law of multiple proportions
32
Who conducted cathode ray experiments?
JJ Thomson
33
What did JJ Thompson discover?
A new particle, which carried a negative electrical charge (electrons)
34
a positive and negative electrical charge will ___ one another
Attract
35
Two positive charges will ____ one another. Two negative charges will also ____ one another
Repel
36
Who conducted an oil drop experiment?
Robert Millikan
37
Robert Millikans experiment determined ___
The exact charge of an electron (-1.60x10^-19C)
38
JJ Thomson proposed the model known as _____
The plum-pudding model
39
Who conducted the gold foil experiment?
Ernest Rutherford
40
What did Ernest Rutherford discover?
He discovered that the plum-pudding model was wrong. Introduced the nuclear model, protons and neutrons, and their electrical charges
41
The nuclear theory of the atom has three basic parts:
1.Most of the atom’s mass and all of its positive charge are contained in a small core called a nucleus. 2.Most of the volume of the atom is empty space, throughout which tiny, negatively charged electrons are dispersed. 3.There are as many negatively charged electrons outside the nucleus as there are positively charged particles (named protons) within the nucleus, so that the atom is electrically neutral.
42
The mass of a neutron is similar to that of a proton. –It has no electrical charge.
Neutron
43
All atoms are composed of the same subatomic particles:
Protons, electrons, neutrons
44
The mass of the proton is
1.67262x10^-27kg
45
The mass of the neutron is
1.67493x10^-27kg
46
The mass of the electron is
9.1x10^-31kg
47
Atoms with the same number of protons but a different number of neutrons are called
Isotopes
48
The sum of the number of neutrons and protons in an atom is its ____
Mass number
49
The number of protons in an atom’s nucleus is its ____
Atomic number
50
What does 20 represent in the following isotope? Ne-20
Mass number
51
Positively charged ions are called ____. They lose electrons
Cations
52
Negatively charged ions are called ____. They gain electrons
Anions
53
What are the atomic number (Z), mass number (A), and symbol of the chlorine isotope with 18 neutrons?
Z = 17, so chlorine has 17 protons. A=number of protons+number of neutrons =17+18=35
54
What are the atomic number, mass number, and symbol for the carbon isotope with 7 neutrons?
55
Atomic mass is sometimes called _______ or standard atomic weight.
Atomic weight
56
we calculate the atomic mass with the following equation:
57
anything containing 6.02214x10^23 pieces is known as a __
Mole
58
What is the number referred to as avogadros number?
6.02214x10^23
59
A substance composed of two or more elements in a fixed, definite proportion is
A compound
60
Two or more substances in variable proportions, where the composition is constant throughout is
Homogeneous mixture
61
Which of the following statements is FALSE according to Daltons Atomic Theory? A. Atoms combine in simple whole number ratios to form compounds. B. All atoms of chlorine have identical properties that distinguish them from other elements. C. One carbon atom will combine with one oxygen atom to form a molecule of carbon monoxide. D. Atoms of sodium do not change into another element during chemical reaction with chlorine. E. An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.
E. An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.
62
Identify the characteristic of a liquid
Definite volume, no definite shape
63
Rutherfords Gold Foil Experiment helped prove
That the mass of an atom is concentrated in a very small space
64
All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?
Law of definite proportions
65
All of the following are SI base units of measurement, EXCEPT: A. kelvin B. Second C. Mole D. Meter E. Gram
E. Gram
66
A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 1.79 g/mL, 1.81 g/mL, 1.80 g/mL, 1.81 g/mL. If the actual value for the density of the sugar solution is 1.80 g/mL, which statement below best describes her results?
Her results are both precise and accurate
67
If a particular process is endothermic, the reverse process must be a (an)
Exothermic process