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GEN CHEM > Lesson 3 > Flashcards

Lesson 3 Flashcards

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1
Q

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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2
Q

-Foundation of stoichiometric calculations
• Allows chemist to determine the amounts of reactants or products involved in a chemical reaction

A

Law of conservation of mass

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3
Q

-Also called the law of definite composition

-Any sample of a given compound will always be composed of the same
elements in the same proportion by mass:

A

Law of definite proportion

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4
Q
  • 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 proportion

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5
Q

Law of multiple proportion
Example: N and 0 can combine to produce different compounds in
different whole number ratio:
A. NO
B. NO2
C. N₂O

A
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6
Q

Dalton’s atomic theory
Book = A new System of Chemical Philosophy
• Proposed an atomic theory of matter that can explain
chemical observations as predicted by the three fundamental laws

A
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7
Q

Dalton atomic theory(READ)
Postulates:
1. Matter is made up of extremely small indivisible particles called atoms.
2. Atoms of the same element are identical and are different from those other elements:
3. Compounds are formed when atoms of different elements combine in certain whole-number ratios
4. Atoms rearrange only during a chemical reaction to form new compounds.

A
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8
Q

-There are various basic elements from which all matter is made -Everything is composed of small atoms moving in a void

A

Democritus(460-370 B.C.)

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9
Q

-Some atoms are round, pointy, oily, have hooks, etc. to account for their properties
-Ideas rejected by leading philosophers because void = no existence

A

Democritus (460-370 B.C.)

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10
Q

-Introduced his ideas in 1803
-Each element is composed of extremely small
-particles called atoms All the atoms of a given element are identical, but
they differ from those of any other element

A

John Dalton (1766-1844)

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11
Q

-Atoms are neither created nor destroyed in any chemical reaction

-A given compound always has the same relative numbers and kinds of atoms

A

John Dalton (1766-1844)

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12
Q

Discovered electron 1897-Cathode Ray Experiment

A

Joseph John Thomson (1856-1940)

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13
Q

-Plum Pudding model 1904
•Electrons in a soup of positive charges

A

Joseph john thomson(1856-1940)

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14
Q

Discovered isotopes 1913

A

Joseph john thomson

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15
Q

Discovery of the Electron In 1897, J.J. Thomson used a cathode ray tube to deduce the presence of a negatively charged particle: the electron

A
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16
Q

Conclusion from the Study of Electron

A. Cathode rays have identical
properties regardless of the element used to produce them. All elements must contain identically charged electrons.

B. Atoms are neutral, so there must be positive particles in the atom to
balance the negative charge of the electrons

C. Electrons have so little mass that atoms must contain other particles that account for most of the mass

A
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17
Q

Nucleus Theory, 1910
•alpha particle gold foil experiment

A

Ernest Rutherford (1871-1937)

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18
Q

-An atom’s mass is mostly in the nucleus
-The nucleus has a positive charge (Moseley)
-Electrons in fixed orbit

A

Ernest Rutherford (1871-1937)

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19
Q

Electrons are

A

Negative charge

20
Q

Proton are

A

Positive charge

21
Q

Neutron are

A

Neutral charge

22
Q

Alpha particle gold foil experiment:
-Particles shot through thin sheet of gold
-Most shots went straight through
-A small amount were deflected
-Hence…. The atoms must be made of mostly empty space with a small dense nucleus

A
23
Q

Rutherford found that most (99%) of the alpha particles that he shot at the gold went straight through

From these experiments Rutherford concluded that the atom had a dense positive core, with the rest composed of mostly empty space with the occasional negatively charged electron

A

Nuclear model

24
Q

Planetary Model 1913
- Nucleus surrounded by orbiting electrons at different energy levels
-electrons exist in several distinct layers or levels
-Electrons have definite orbits

A

Niels Bohr (1885-1962)

25
Q

• Travel around nucleus like planets around sun travel

• Electrons can jump between levels with energy being added/released

A

Niels Bohr (1885-1962)

26
Q

Quantum Mechanical Model 1926

• Electrons are in probability zones called “orbitals, not orbits and the location cannot be pinpointed
•Electrons are particles and waves at the same time
• Developed quantum numbers based on theories of Einstein and Planck

A

Ernst Schrödinger 1887-1961 and
Werner Heisenberg 1901-1976

27
Q

Quantum Mechanical Model

•Found that Electrons live in fuzzy regions or “clouds” not distinct orbits

•Improved on Bohr’s findings
Electron location can not be predicted the current understanding of the atom is based on Quantum Mechanics

•this model sees the electrons not as individual particles, but as behaving like a cloud- the electron can be “anywhere” in a certain energy level

A

Quantum mechanical model

28
Q

Who discovered protons

A

Eugene goldstein

29
Q

Who discovered electron

A

James chadwick

30
Q

is the weighted average mass of all the atomic masses of the isotopes of that atom

A

Atomic mass

31
Q

Hydrogen exists with three isotopes, namely

A

Protium 1.1
Deuterium 2.1
Tritium 3.1

32
Q

is an atom, or group of atoms, that has a net positive or negative charge

A

Ion

33
Q

Ion with positive a charge

A

Cation

34
Q

Ion with negative charge

A

Anion

35
Q

If a neutral atom loses one or
more electrons

A

Cation

36
Q

If a neutral atom gains one or more electrons

A

Anion

37
Q

ion contains only one atom
Example:
Al, Ca3

A

Monatomic

38
Q

ion contains more than one atom
Example:
OH, NH, NO

A

Polyatomic

39
Q

is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds

A

Molecules

40
Q

contains only two atoms

A

Diatomic molecule

41
Q

contains more than two atoms

A

Polyatomic molecule

42
Q

is a notation used by scientists to show the number and type of atoms present in a molecule, using the atomic symbols and numerical subscripts. A chemical formula is a simple representation, in writing, of a three-dimensional molecule that exists. A chemical formula describes a substance, down to the exact atoms which make it up. (Example: H₂O, NO)

A

Chemical formula

43
Q

comes in to show the actual number of atoms within each molecule.

A

Molecular formula

44
Q

-represents the relative/simplest number of atoms of each element in the compound. Some compounds, like water, have the same empirical and molecular formula, because they are small and have the same ratio of atoms in molecules and number of atoms in a molecule.

A

Empirical formula

45
Q

the actual bonds between molecules are shown. This helps the reader understand how the different atoms are connected, and thus how the molecule functions in space

A

Structural formula

GEN CHEM (4 decks)

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