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Chemistry > CHE128 Chapter 4 > Flashcards

CHE128 Chapter 4 Flashcards

1
Q

What was Dalton’s Atomic Theory?

A

Each element was made of tiny, hard, indivisible spheres called atoms, and that all atoms of an element are identical.

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2
Q

What is a Dalton sometimes called?

A

AMU (atomic mass unit)

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3
Q

What was Thomson’s Plum Pudding Model?

A

That electrons were suspended in a positively charged electric field. Because there was no evidence of positive matter, he assumed there must be positive energy.

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4
Q

How did Rutherford test the Plum Pudding Model?

A

Shot alpha particles (as bullets) through the atoms (of gold foil). 98% went straight through. 2% went through but were deflected, and 0.01% bounced off the gold foil.

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5
Q

What are the three main components of an atom?

A

Proton (+), Neutron (=), Electron (-)

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6
Q

What number is equal to the number of protons in an atom?

A

Atomic number

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7
Q

What number is equal to the number of protons and neutrons in an atom?

A

Atomic mass

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8
Q

Define Atomic number.

A

The number of protons in an atom. (shorthand: Z)

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9
Q

Define Atomic Mass

A

The mass of an atom; protons + neutrons (shorthand, A)

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10
Q

Why aren’t electrons considered in atomic mass?

A

Their mass is tiny - virtually zero.

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11
Q

If a neutral atom has 20 protons, how many electrons will it have?

A

20 electrons

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12
Q

If a proton has 20 protons and 20 neutrons, what is its atomic mass?

A

40 amu

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13
Q

If an atom has 20 protons and 18 electrons, what is its charge?

A

+2

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14
Q

What is Periodic Law?

A

Stated by Mendeleev: When elements are arranged in order of increasing mass, properties recur periodically

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15
Q

Where do metals fall on the Periodic Table?

A

Most of the left side (excluding H)

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16
Q

Where do metalloids fall on the Periodic Table?

A

In a diagonal pattern between metals and nonmetals.

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17
Q

Where are non-metals on the periodic table?

A

The right side of the table (plus H)

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18
Q

Describing a Metal or nonmetal: Shiny

A

Metal

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19
Q

Describing a Metal or nonmetal: Conducts heat and electricity

A

Metal

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20
Q

Describing a Metal or nonmetal: Malleable

A

Metal

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21
Q

Describing a Metal or nonmetal: Ductile

A

Metal

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22
Q

Describing a Metal or nonmetal: Found in all 3 states

A

Non-metal

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23
Q

Describing a Metal or nonmetal: Poor conductor of heat and electricity.

A

Non-metal

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24
Q

Describing a Metal or nonmetal: Brittle

A

Non-metal

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25
Q

Describing a Metal or nonmetal: Gains electrons to become anions

A

Non-metal

26
Q

What types of elements show some properties of metals and some of non-metals?

A

Metalloids

27
Q

What are columns called in the periodic table?

A

Groups or Families

28
Q

What are rows called in the periodic table?

A

Periods

29
Q

Name the Group #: Alkali Metals

A

Group 1A

30
Q

Name the Group #: Alkali Earth Metals

A

Group 2A

31
Q

Name the Group #: Transition Metals

A

Groups 3B through 2B (3-12 overall)

32
Q

Name the Group #: Halogens

A

Group 7A

33
Q

Name the Group #: Noble Gasses

A

Group 8A

34
Q

Name three properties of Hydrogen.

A

Non-metal, Colorless gas, Reacts with non-metals to form molecular compounds, reacts with metals to form hydrides.

35
Q

Name three properties of Alkali Metals.

A

Group 1A, soft, low melting points, flame tests, very reactive

36
Q

Name three properties of Alkali Earth Metals.

A

Group 2A, slightly harder, higher melting, and denser than alkali metals, flame tests, less reactive than alkali metals

37
Q

Name three properties of halogens.

A

Group 7A, nonmetal, diatomic, very reactive, reacts with metals to form ionic compounds

38
Q

Name three properties of noble gasses.

A

Group 8A, all gasses at room temp, very unreactive

39
Q

What is an Ion?

A

atoms which are electrically charged because of having gained or lost electrons.

40
Q

How can you calculate ionic charge?

A

of protons minus # of electrons

41
Q

Cation: positive or negative charge?

A

Positive (less electrons)

42
Q

Anion: positive or negative charge?

A

Negative (gained electrons)

43
Q

Do non-metals form anions or cations?

A

anions

44
Q

A fluorine anion has its suffix named to what?

A

-ide (to form flouride)

45
Q

Do metals form anions or cations?

A

Cations

46
Q

A sodium ion has its name changed how?

A

The word ion is added at the end - sodium ion.

47
Q

What are Valence Electrons?

A

The highest energy electrons in an atom

48
Q

Elements with different masses due to varying number of neutrons are called what?

A

Isotopes

49
Q

How is average atomic mass calculated?

A

(mass of 1st isotope X frequency of 1st isotope) + (mass of second isotope X frequency of second isotope)

50
Q

Do different isotopes undergo different chemical reactions?

A

Nope - All isotopes are chemically identical.

51
Q

Do isotopes have different numbers of protons?

A

No

52
Q

Do different isotopes have different masses?

A

Yes - mass is determined by protons + neutrons.

53
Q

How can we infer the number of neutrons an atom has?

A

Subtract the number of protons (atomic number) from the atomic mass.

54
Q

What is the difference between mass number and atomic mass?

A

Mass number refers to the # of protons + neutrons in one isotope; Atomic mass is an experimental number determined from All naturally occurring isotopes. Mass number will always be a whole number.

55
Q

What was Rutherford’s interpretation of the Atom called?

A

The Nuclear Model

56
Q

Describe Rutherford’s Nuclear Model.

A

Atom contains a tiny dense center called the nucleus, which has the entire mass of the atom and is positively charged. Electrons are dispersed in the empty space surrounding the nucleus.

57
Q

What were two problems with Rutherford’s Nuclear Model?

A

1) How do protons stick together in the nucleus? Shouldn’t they repel? 2) An atom with 4 protons should weight 4 amu, but it weighs 9 amu

58
Q

What did Rutherford propose as an addition to his Nuclear Model?

A

That Neutrons were also inside the nucleus, with a mass of 1 amu

59
Q

What were some errors in Dalton’s Atomic Theory?

A

That all elements of an atom are identical in mass, and that atoms are “unbreakable”

60
Q

Who discovered that atoms had pieces called Electrons?

A

J.J. Thomson

61
Q

What could Rutherford conclude from his “plum pudding” experiment?

A

Atoms are mostly empty space; Atoms contain a dense particle small in volume but large in mass, and this dense particle was positively charged.

Chemistry (3 decks)

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