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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
a key postulate in Dalton's Atomic Theory where he believed atoms could not be created, destroyed, or divided into smaller parts.
1. All matter is composed of tiny, indivisible particles called atoms.
26
a key postulate in Dalton's Atomic Theory where he stated that all atoms of a given element are identical to one another.
2. Atoms of the same element are identical in size, mass, and other properties.
27
a key postulate in Dalton's Atomic Theory where each element consists of its unique type of atom with distinct characteristics.
3. Atoms of different elements differ in size, mass, and properties.
28
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).
4. Atoms combine in simple whole-number ratios to form compounds.
29
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.
5. Chemical reactions involve the rearrangement of atoms.
30
the subatomic particles
electron nucleus - proton - neutron
31
________________ discovered electron while studying _____________
Joseph John Thompson (1856 - 1940) cathode ray tube
32
Proposed the “Plum-Pudding model”
Joseph John Thompson
33
_____________ performed the _____________
Ernest Rutherford gold foil experiment
34
Discovered proton
Ernest Rutherford
35
Discovered neutron
James Chadwick
36
Planetary model
Neils Bohr
37
atoms with the same element but with different numbers
isotopes
38
an atom or a molecule that has gained or lost on or more electrons, resulting to a net electrical charge
Ions
39
metals tend to lose electrons and become positively charged
cations
40
nonmetals gain electrons and become negatively charges
anions
41
the metal elements
1. alkali metals (group 1) 2. alkaline metals (group 2) 3. transition metals (group 3-12) 4. lanthanides (rare earth metals)
42
a metal element that are highly reactive, especially with water; soft metals w/ low melting points
alkali metals (group 1)
43
a metal element that are less reactive than alkali metals but still reactive, harder metals, higher melting points than alkali metals
alkaline metals (group 2)
44
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
transition metals (group 3-12)
45
a metal element that are often referred to as rare earth metals, used in electronics and strong magnets, typically have higher luster and conductivity
lanthanides (rare earth metals)
46
how to find mass #
#protons + #neutrons
47
how to find atomic #
= #protons
48
how to find # neutrons
mass # - atomic #
49
Many are radioactive; some are used in nuclear energy applications.
Actinides
50
Softer than transition metals, often have lower melting and boiling points, still conduct heat and electricity but less effectively.
Post-Transition Metals
51
Location: Far left periodic table column (excluding hydrogen).
Alkali Metals (Group 1)
52
Location: Second column from the left.
Alkaline Earth Metals (Group 2)
53
Location: The large block in the middle of the periodic table.
Transition Metals (Groups 3-12)
54
Location: The first row of the two rows below the main periodic table.
Lanthanides (Rare Earth Metals)
55
Location: The second row of the two rows below the main periodic table.
Actinides
56
Location: Just to the right of the transition metals.
Post-Transition Metals
57
Location: Found along the dividing line (the "staircase") between metals and non-metals.
Metalloids
58
Properties: These elements have properties of both metals and non-metals.
Metalloids
59
consists of only one atom
MONOATOMIC ION
60
combinations of different atoms
POLYATOMIC ION
61
formed between metals and nonmetals.
Ionic compounds
62
formed between two nonmetals.
Covalent Compounds

GENERAL CHEMISTRY 1 (2 decks)

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