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GENERAL CHEMISTRY 1 > Fundamental Laws of Chemistry > Flashcards

Fundamental Laws of Chemistry Flashcards

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1
Q

book published by Robert Boyle

A

The Sceptical Chymist

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2
Q

defines the simplest composition of matter that cannot be broken down further by any chemical means

A

The Sceptical Chymist

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3
Q

atoms of elements combine to form different compounds

A

The Sceptical Chymist

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4
Q

year Robert Boyle published his book

A

1661

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5
Q

In this book,
 It questioned traditional approaches
 Introduced a new way of thinking about chemical substances and reactions.
 He emphasizes the importance of experimentation, observation, & understanding the nature of matter.

A

The Sceptical Chymist

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6
Q

Boyle challenged the____________ theories that all substances were composed of __ elements

A

Aristotelian
4

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7
Q

___________ is a scientist who isolated the oxygen gas which he called ___________ by heating ______________

A

Joseph Priestley
dephlogisticated air
mercury oxide

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8
Q

when did Priestley discover dephlogisticated air

A

1774

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9
Q

he invented carbonated water in 1772

A

Joseph Priestley

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10
Q

he is a French chemist and the Father of Modern Chemistry.

A

Antoine-Laurent Lavoisier

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11
Q

Lavoisier found out that the gas, which he already called oxygen, is involved in _____________________.

A

combustion and respiration

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12
Q

he invented the Law of Conservation of Mass

A

Antoine-Laurent Lavoisier

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13
Q

states that in a chemical reaction, the mass of the substances produced is equal to the mass of the substances reacted.

A

Law of Conservation of Mass

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14
Q

He named the elements oxygen, hydrogen and other elements.

A

Antoine-Laurent Lavoisier

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15
Q

measured the amount of the substances before and after a chemical reaction in a closed vessel. His data led him to conclude that matter can undergo changes during a chemical reaction, but the total mass of the substances involved in the reaction is constant.

A

Antoine-Laurent Lavoisier

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16
Q

 A 100-gram water sample contains 89% oxygen and 11% hydrogen by mass 100 kilograms of water also contains the same percentages by mass. This is an example of _______________

A

Law of Definition Proportion/Composition

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17
Q

In whatever form it is used, nitrous oxide is always composed of 64% nitrogen and 36% oxygen by mass. This is an example of _______________

A

Law of Definition Proportion/Composition

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18
Q

also known as laughing gas, nitrous or nitro

A

Nitrous oxide (N₂O)

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19
Q

uses of Nitrous oxide (N₂O)

A

dental analgesic, anesthetic, engine

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20
Q

made the Law of Definition Proportion/Composition

A

Joseph-Louis Proust

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21
Q

states that any sample of given compound will always be composed of the same element in the same proportion by mass

A

Law of Definition Proportion/Composition

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22
Q

a British scientist that made the Law of Multiple Proportions

A

John Dalton

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23
Q

states that for elements that can form different compounds, the masses of the second element that can combine with a fixed mass of the first element are in a ratio of small whole numbers.

A

Law of Multiple Proportions

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24
Q

Example: carbon and oxygen can combine to form two different compounds -carbon monoxide (CO) and carbon dioxide (CO₂).
 In forming CO, 5 g of carbon combines with 6.7 g of oxygen;
 while in forming CO₂, 5.0 grams of carbon combines with 13.3 grams of oxygen.
o The ratio of masses of oxygen that combines with the same amount of carbon is 6.7:13.3, or simply about 1:2.

A

Law of Multiple Proportions

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25
Q

a key postulate in Dalton’s Atomic Theory where he believed atoms could not be created, destroyed, or divided into smaller parts.

A
  1. All matter is composed of tiny, indivisible particles called atoms.
26
Q

a key postulate in Dalton’s Atomic Theory where he stated that all atoms of a given element are identical to one another.

A
  1. Atoms of the same element are identical in size, mass, and other properties.
27
Q

a key postulate in Dalton’s Atomic Theory where each element consists of its unique type of atom with distinct characteristics.

A
  1. Atoms of different elements differ in size, mass, and properties.
28
Q

a key postulate in Dalton’s Atomic Theory where compounds are composed of atoms of different elements combined together in fixed ratios (e.g., H₂O, CO₂).

A
  1. Atoms combine in simple whole-number ratios to form compounds.
29
Q

a key postulate in Dalton’s Atomic Theory where in chemical reactions, atoms are neither created nor destroyed but are rearranged to form new compounds.

A
  1. Chemical reactions involve the rearrangement of atoms.
30
Q

the subatomic particles

A

electron
nucleus - proton
- neutron

31
Q

________________ discovered electron while studying _____________

A

Joseph John Thompson (1856 - 1940)
cathode ray tube

32
Q

Proposed the “Plum-Pudding model”

A

Joseph John Thompson

33
Q

_____________ performed the _____________

A

Ernest Rutherford
gold foil experiment

34
Q

Discovered proton

A

Ernest Rutherford

35
Q

Discovered neutron

A

James Chadwick

36
Q

Planetary model

A

Neils Bohr

37
Q

atoms with the same element but with different numbers

A

isotopes

38
Q

an atom or a molecule that has gained or lost on or more electrons, resulting to a net electrical charge

A

Ions

39
Q

metals tend to lose electrons and become positively charged

A

cations

40
Q

nonmetals gain electrons and become negatively charges

A

anions

41
Q

the metal elements

A
  1. alkali metals (group 1)
  2. alkaline metals (group 2)
  3. transition metals (group 3-12)
  4. lanthanides (rare earth metals)
42
Q

a metal element that are highly reactive, especially with water; soft metals w/ low melting points

A

alkali metals (group 1)

43
Q

a metal element that are less reactive than alkali metals but still reactive, harder metals, higher melting points than alkali metals

A

alkaline metals (group 2)

44
Q

a metal element that are typically good conductors of heat and electricity, malleable, ductile, often formed colored compounds, many are used in industry and jewelry

A

transition metals (group 3-12)

45
Q

a metal element that are often referred to as rare earth metals, used in electronics and strong magnets, typically have higher luster and conductivity

A

lanthanides (rare earth metals)

46
Q

how to find mass #

A

protons + #neutrons

47
Q

how to find atomic #

A

= #protons

48
Q

how to find # neutrons

A

mass # - atomic #

49
Q

Many are radioactive; some are used in nuclear energy applications.

A

Actinides

50
Q

Softer than transition metals, often have lower melting and boiling points, still conduct heat and electricity but less effectively.

A

Post-Transition Metals

51
Q

Location: Far left periodic table column (excluding hydrogen).

A

Alkali Metals (Group 1)

52
Q

Location: Second column from the left.

A

Alkaline Earth Metals (Group 2)

53
Q

Location: The large block in the middle of the periodic table.

A

Transition Metals (Groups 3-12)

54
Q

Location: The first row of the two rows below the main periodic table.

A

Lanthanides (Rare Earth Metals)

55
Q

Location: The second row of the two rows below the main periodic table.

A

Actinides

56
Q

Location: Just to the right of the transition metals.

A

Post-Transition Metals

57
Q

Location: Found along the dividing line (the “staircase”) between metals and non-metals.

A

Metalloids

58
Q

Properties: These elements have properties of both metals and non-metals.

A

Metalloids

59
Q

consists of only one atom

A

MONOATOMIC ION

60
Q

combinations of different atoms

A

POLYATOMIC ION

61
Q

formed between metals and nonmetals.

A

Ionic compounds

62
Q

formed between two nonmetals.

A

Covalent Compounds

GENERAL CHEMISTRY 1 (2 decks)

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