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Chem 104 > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

chemistry

A

the study of the composition and structure of matter and of the changes that matter undergoes

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2
Q

matter

A

Whatever occupies space and can be percieved by our senses

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3
Q

mass

A

The quantity of matter

The quantity of matter is conserved

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4
Q

The Law of Conversion of Mass

A

No mass is lost from the start of a process to the end

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5
Q

extensive property (of matter)

A

a property that depends on the amount of substance (mass, volume, etc.)

Extensive properties are a physical property of matter

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6
Q

intensive property of matter

A

a property of matter that does not depend on the amount of substance (color, melting point, density)

Intensive properties are physical properties of matter

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7
Q

Physical property of matter

A

Can be observed without doing a chemical reaction (luster, hardness, color)

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8
Q

Chemical property of matter

A

Property that can be observed through chemical reaction (flammability, reactivity, etc)

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9
Q

Pure Substance

A
  • Same physical and chemical properties throughout
  • Cannot be separated into simpler substances by a physical process

ex. elements, compounds

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10
Q

Mixture

A
  • Combination of two or more pure substances
  • Can be separated by physical processes
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11
Q

Element

A

A pure substance that cannot be separated into simpler substance by any chemical process

This includes diatomic and polyatomic molecules w only one element

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12
Q

Common Diatomic Molecules

A

Br I N Cl H O F

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13
Q

Common Polyatomic Molecules

A

P and S

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14
Q

Compounds

A
  • Pure substance composed of two or more different elements bonded together in fixed proportions (ex. water, carbon dioxide)
  • Compounds can be broken down into individual elements via chemical means
  • All samples of a particular compound contain the same elements combined in the same proportions (The Law of Constant Composition/Law of Definite Proportions)

The chemical formula denotes the elements and their respective proportions in a given compound. If these proportions change, the compound has changed.

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15
Q

The Law of Constant Composition/ The Law of Definite Proportions

A

All samples of a particular compound contain the same elements combined in the same proportions

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16
Q

Homogeneous Mixtures

A

Components are distributed uniformly through the sample and have no visible boundaries or regions

Ex. sugar in coffee

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17
Q

Heterogeneous Mixtures

A

Components are not distributed uniformly, and there may be distinct regions with different compositions

Ex. sand in water

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18
Q

Plasma

A

A state of matter, superheated matter similar to a gas, but made up entirely of charged particles

19
Q

Lavoisier 1789

A
  • The law of multiple proportions and mass cannot be created/destroyed
  • If two elements can form more than one compound together, the ratio of the masses of the second element will always be a whole number when combining with a fixed mass of the first element

Eg. CO and CO2 (same amount of carbon, whole number ratio b/w oxygen and carbon)

20
Q

Dalton 1807

A
  • Atoms are indestructible+ Atomic Theory+ Law of Multiple Proportions
21
Q

Atomic Theory (Dalton 1807)

A
  1. Matter is composed of atoms, the smallest particle capable of participating in chemical reactions
  2. Elements contain only one type of atom, characteristic of that particular element
  3. Atoms of one element have different properties than atoms of other elements
  4. Law of definite proportions
  5. Atoms are neither created nor destroyed during a chemical reaction, but are rearranged
22
Q

Mendeleev-1869

A

Arranged the elements to form the Periodic Table of Elements

23
Q

Goldstein 1885

A
  • Discovered positive particles
24
Q

Thomson 1897

A

Discovered the electron using cathode rays, developed the plum pudding model

25
Q

Rutherford 1907

A
  • Gold foil experiment
  • Alpha particles used to bombard gold foil, mass discovered at the center of the atom
  • The atom itself is mostly empty space
26
Q

Milikan-1909

A

Determined the mass and charge of an electron with the oil drop experiment

27
Q

Bohr 1913

A

Electrons orbiting in shells around the nucleus, can be excited and move to higher energy orbitals

28
Q

Heisenberg 1925

A

Uncertainty principle: You cannot know the energy and location of an electron at the same time

29
Q

Chadwick-1932

A

Discovered the neutron, necessary to balance the positive nucleus

30
Q

Atomic Mass Units (amu)

A
  • unit used to express the relative masses of atoms and subatomic particles
  • Carbon 12= 12 amu (6 protons + 6 neutrons)
  • 1 amu =1 dalton (Da)
31
Q

The Modern Periodic Table Periods

A
  • Period 1: Alkali Metals
  • Period 2: Alkaline Earth Metals
  • Period 17: Halogens
  • Period 18: Noble Gases
32
Q

Metals Characteristics

A
  • Shiny solids (besides Hg)
  • Conduct heat and electricity
  • Are malleable
33
Q

Nonmetals characteristics

A
  • Solids, liquids, and gases
  • Nonconductors
  • The solids are brittle
34
Q

Metalloids

A
  • shiny solids (like metals)
  • brittle (like nonmetals)
  • semiconductors
35
Q

Aston-1919

A
  • Aston developed a mass spectrometer, which showed through experimentation that two different masses of neon gas exist
36
Q

Ions

A
  • Neutral atoms that gain/lose electrons become ions
  • Ions are held together by electrostatic force (opposites attract)
37
Q

Cation vs. anion

A
  • Cations have a positive charge (less electrons than normal)
  • Anions have a negative charge (more electrons than normal)
38
Q

Ionic Compounds

A
  • Made from a metal and a nonmetal
  • Metals form cations; nonmetals form anions
  • Charges depend on periodic table location
39
Q

formula unit

A

the smallest electrically neutral unit of an ionic compound

40
Q

Molecular compounds

A

Composed of atoms held together in molecules by covalent bonds and are composed of nonmetals

41
Q

Covalent bonds

A

Bond between two atoms created by sharing one or more pairs of electrons

42
Q

Molecular formula

A

Shows the number and type of atoms present in one molecule of a compound

43
Q

Empirical formula

A

Shows the smallest whole-number ratio of elements in a compound

Chem 104 (20 decks)

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