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Chem 120 > Exam #1 > Flashcards

Exam #1 Flashcards

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1
Q

What is a proposed explanation of fact that cannot be tested through experiment?

A

Hypothesis

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2
Q

What is a proven hypothesis generally accepted with evidence or data to support it?

A

Theory

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3
Q

What is a statement of natural phenomena with no exception?

A

Scientific law

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4
Q

These are a unique classification of matter.

A

Elements

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5
Q

This is a column of the periodic table and consist of elements with similar properties.

A

Groups

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6
Q

This is a horizontal row on the periodic table.

A

Period

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7
Q

What are the three groups elements are separated into?

A

Metals, non-metals, and metalloids

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8
Q

Semiconductors; conduct heat under certain conditions

A

Metalloid

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9
Q

Usually solids, liquids, or gases at room temperature; not lustrous and poor conductors of electricity

A

Non-metals

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10
Q

Lustrous, conduct electricity, malleable, and usually solid at room temperature

A

Metals

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11
Q

What are the 5 groups of metals?

A

Alkali, alkaline earth metals, transition metals, halogens, and noble gases

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12
Q

Soft, reactive, combust with contact of water ; first column

A

Alkali

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13
Q

Relatively soft and relatively reactive; second column

A

Alkaline earth metals

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14
Q

Typical, everyday metals; Sc to zn

A

Transition metals

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15
Q

Very reactive

A

Halogens

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16
Q

Unreactive!

A

Noble gas

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17
Q

Is hydrogen considered an alkali metal?

A

No.

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18
Q

Units made of two or more other units; example: density= mass/volume

A

Derived unit

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19
Q

If we have a whole number and want to write it in scientific notation, do we more it to the left since it’s positive?

A

Yes; example: 101,325 = 1.01325 x 10^5

20
Q

If we have a decimal and want to write it in scientific notation, will we go left or right?

A

Right; example: 1.01325 = 101,325 x 10^-5

21
Q

What are the formulas for temperature conversion?

A

Celsius= (f-32)x 5/9
Kelvin = C+ 273.15

22
Q

List the multiplicative prefixes in order with measurements.

A

Nano (n)- 10^-9
Micro (u)- 10^ -6
Milli (m)- 10^-3
Centi (c)- 1/100; 0.01
Deci(d)- 1/10; 0.1
Kilo (k)- 10^3
Mega (M)- 10^6
Giga (G)- 10^9

23
Q

Macroscopic and particulate models

A

Macroscopic: level you can see matter with naked eye
Particulate: need models or specialized tool to visualize matter; microscopic

24
Q

This phase of matter has a definite volume, define shape, and low particle motion

A

Solid

25
Q

This phase of matter has definite volume, no definite shape, and has high particle motion that is limited by volume

A

Liquid

26
Q

This phase of matter is compressible, has no definite shape or volume, and has very high particle motion

A

Gas

27
Q

This describes the motion of matter at a particulate level

A

Kinetic molecular theory

28
Q

Are pure substances one form of matter? Give 2 examples.

A

Yes; elements and compounds

29
Q

Are mixtures 2 or more forms of matter? What are the 2 types? Give examples.

A

Yes; homogeneous, which is every mixed, and heterogeneous, which is distinguishable is composition.

Examples: homogeneous- brass, soda water; heterogeneous- treasure, tapioca milk lea

30
Q

What are the 2 ways to separate mixtures?

A

Distillation and filtration, to name a few

31
Q

Separation of 2 substances with phase change; useful for homogenous mixtures

A

Distillation

32
Q

Separation of 2 substances through semipermeable barrier; good for heterogeneous mixtures

A

Filtration

33
Q

What are the 2 types of changes substances can undergo?

A

Physical and chemical

34
Q

A change that occurs with no change in chemical compound

Example: melting ice, cutting something in half

A

Physical property

35
Q

Property that alter chemical composition of a source of matter

Example: burning paper, iron rusting

A

Chemical property

36
Q

What does the law of conservation of matter state?

A

Matter is with created nor destroyed; mass should not differ after reaction

37
Q

The capacity for matter to do work; resource absorbed or released; detected as heat or work

A

Energy

38
Q

Energy of an object due to its relative position or stored energy

A

Potential energy

39
Q

Energy released by movement

A

Kinetic energy

40
Q

The law that energy is neither created nor destroyed, but absorbed or released

A

Law of conservation of energy

41
Q

T/f: unlike charges repel and like charges attract

T/f: like charges put together build potential energy

A

False; unlike charges attract and like charges repel

True

42
Q

Who proposed that all atoms of an element have the same mass and size, which has been proven to be false, and that atoms were hard spheres, which was also disproved.

A

Dalton

43
Q

Who proposed the plum pudding model, which was disproved, that resulted in discovery of the electron.

A

Thomson

44
Q

Who dealt with alpha particles and shot them expecting them to deflect, but they went straight through. He discovered the nucleus.

A

Rutherford

45
Q

Explain the structure of an atom.

A

Nucleus is center with protons, and electrons on outside: all within atom

46
Q

An element of a particular atomic number that duffers in number of neutrons.

Mass number is the sum of protons and neutrons

Atomic number: number of protons and electrons in nucleus

A

Isotope

Chem 120 (1 decks)

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