Ch 3 Section 1 Flashcards

1
Q

Democritus called natures basic particle an

A

Atom based on Greek word meaning “indivisible”

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2
Q

Aristotle thought that all matter was

A

Continuous and his opinion was accepted for nearly 2000 years

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3
Q

Neither the view of Aristotle nor that of Democritus was supported by

A

Experimental evidence do each remained speculation until the 18th century

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4
Q

Virtually all c he jets in the late 1700s accepted the modern definition of an element as a

A

Substance that cannot be further broken down by ordinary chemical means

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5
Q

It was clear that elements combine to form

A

Compounds that have different physical and chemical properties than those of the elements that form them

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6
Q

Great controversy as to whether elements

A

Always combine in the same ratio when forming a compound

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7
Q

Chemical reaction

A

Transformation of a substance(s) into one or more new substance

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8
Q

Particle theory of matter was was supported as early as

A

400 BC by Greek thinkers such as Democritus

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9
Q

Study of matter was revolutionized by a new emphasis on the

A

Quantitative analysis of chemical reactions

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10
Q

Aided by improved balances investigators began to

A

Accurately measure the masses of elements and compounds

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11
Q

Measurement of masses of elements and compounds led to the discovery of

A

Several basic laws

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12
Q

Law of conservation of mass

A

Mass is neither created nor destroyed during ordinary chemical reactions or physical changes

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13
Q

Discovery followed by assertion that regardless of where or how a pure chemical compound is prepared it is

A

Composed of a fixed proportion of elements

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14
Q

Law of definite proportions

A

Fact that a chemical compound contains the same elements in exCtly the same proportions by mass regardless of size of sample or source of compound

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15
Q

Known that 2 elements sometimes combine to form

A

More than one compound

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16
Q

Law of multiple proportions state that if two or more different compounds are composed of the same 2 elements then the ratio of the

A

Masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

17
Q

Dalton in 1808 proposed an explanation for the

A

Law of conservation of mass
The law of definite proportions
The law of multiple proportions

18
Q

Dalton stated that elements were composed of

A

Atoms and that only whole numbers of atoms can combine to form compounds

19
Q

(Daltons theory) all matter composed of extremely

A

Small particles called atoms

20
Q

(Daltons theory) atoms of a given element are

A

Identical in size mass and other properties

21
Q

(Daltons theory) atoms of different elements differ in

A

Size mass and other properties

22
Q

(Daltons theory) atoms cannot be

A

Subdivided created or destroyed

23
Q

(Daltons theory) atoms of different elements combine in

A

Simple whole number ratios to form chemical compounds

24
Q

(Daltons theory) in chemical reactions atoms are

A

Combined separated or rearranged

25
Q

According to dalton a theory the law of conservation of mass is explained by the fact that chemical reactions merely involve the

A

Combination separation or rearrangement of atoms and that during these processes atoms are not subdivided created or destroyed

26
Q

Law of definite proportions results from the fact that a given chemical compound is always composed of the

A

Same combination of atoms

27
Q

In the case of carbon oxides for law of multiple proportions, 2 to 1 ratio of oxygen masses results because CO2 always contains

A

Twice as many oxygen atoms as does carbon monoxide

28
Q

By relating atoms to measurable property of mass dalton turned Democritus idea into a

A

Scientific theory that could be tested by experiment

29
Q

Today we know that atoms are

A

Divisible into even smaller particles

30
Q

We also know that a given element can have

A

Atoms with different masses

31
Q

Daltons ideas that remain unchanged:

A

All matter is composed of atoms

Atoms of any one element differ in properties from atoms of another element