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Chemistry > Matter > Flashcards

Matter Flashcards

(62 cards)

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1
Q

Pure substance

A

Matter that is made up of only one type of particle.
Ex. Copper (Cu)

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2
Q

Mixture

A

Two or more pure substances mixed together.
Each substance retains its own set of chemical and physical properties.
Unlike pure substances, mixtures can ALWAYS be separated by physical means.
Ex. Salt water

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3
Q

Pure Substance - Elements

A

Substances made up of one type of atom.
Can NOT be separated by any physical or chemical process.
Ex. Gold (Au), Carbon (C), etc.

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4
Q

Elements - Metals

A

Gray, shiny, can be shaped, conductors, and mostly solid.

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5
Q

Elements - Nonmetals

A

Dull, colorful, brittle, insulators, and can be solid, liquid, or gas.

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6
Q

Pure substances - Compounds

A

Particles made of two or more different atoms chemically bonded together.
Ex. Carbon Dioxide (CO2), Water (H2O), etc.
Compounds have only one set of properties.
They can NOT be separated by any physical means.
Can ONLY be separated by a chemical reaction.
All compounds can be written as a chemical formula.

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7
Q

Polyatomic Ions

A

Compounds that have an electrical charge.
Written in the upper right corner of an compound in chemical formulas.

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8
Q

Covalent Compounds

A

A compound made of 2 nonmetals.

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9
Q

Ionic Compounds

A

A compound made of 1 metal and 1 nonmetal.

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10
Q

Mixture - Heterogeneous

A

A mixture that is NOT uniform (hetero = different).
You can see the different parts.

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11
Q

Suspencion

A

When a heterogeneous mixture is left alone and separates it is known as suspencion.

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12
Q

Colloid

A

When a heterogeneous mixture is left alone and does not separate it is known as a colloid.

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13
Q

Mixture - Homogeneous

A

A mixture that is uniform (homo = same)
Can not see the different particles.
AKA a solution.

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14
Q

Compounds vs. Mixtures

A

Compounds -
Homogeneous
Separated by chemical means
Different properties from its components
Definite compositions (H2O2)

Mixtures -
Homogeneous OR heterogeneous
Separated by physical means
Components retain their properties
No definite composition (little salt + lots of water = salt water, lots of salt + little water = salt water)

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15
Q

Physical Properties

A

Properties that can be observed or measured.
Ex. Color, shape, size, odor, mass, melting / boiling point, etc.
Two types of phys. prop. intensive, and extensive.

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16
Q

Intensive Phys. Prop.

A

Property that DOES NOT change with the amount of substance present.
Ex. Color, density, texture, melting / boiling point.

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17
Q

Extensive Phys. Prop.

A

Property that DEPEND ON the amount of matter present.
Ex. Mass, size, volume.

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18
Q

Chemical Properties

A

How a substance reacts with another substance.
Ex. Flammability, reactivity to acids, ability to rust, etc.

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19
Q

States of Matter - Solids

A

Particles packed close together
Particles are organized
Particles have fixed position
Definite shape and volume
Vibrating and rotating motion

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20
Q

States of Matter - Liquids

A

Particles are farther apart than solids
Particles are free to slide past one another, able to flow
Particles have higher energy that solids
Definite volume, no definite shape

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21
Q

States of Matter - Gases

A

Particles very far apart from each other
Particles travel in a random manner
Particles have the highest energy
No definite shape or volume
Low density
Compressible

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22
Q

Phase Changes - Melting

A

Solid —–> Liquid

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23
Q

Phase Changes - Freezing

A

Liquid —–> Solid

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24
Q

Phase Changes - Evaporation

A

Liquid —–> Gas

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25
Phase Changes - Condensation
Gas -----> Liquid
26
Phase Changes - Sublimation
Solid -----> Gas
27
Phase Changes - Deposition
Gas -----> Solid
28
Endothermic
A phase change that absorbs heat Ex. Melting, evaporating, sublimation
29
Exothermic
A phase change that releases heat Ex. Freezing, condensation, deposition
30
Physical Change
Does NOT change the chemical composition (chemical formula) Ex. Phase changes, dissolving, separation of mixtures
31
Seperation - Filtration
Separates a mixture by the size of the particles
32
Seperation - Distillation
Separates a mixture by boiling points
33
Chemical Change
AKA reactions Chemical bonds are broken and reformed into new compounds Can be written as an equation Ex. H2 + O2 ---> H2O
34
Signs of a chemical change
Change of color Effervescent (forms a gas) Forms a precipitate (a solid that can not dissolve) Temperature change
35
"Billiard Ball Model" - Dalton's Atomic Theory (1803)
Atoms are small, solid, dense, and spherical Atoms make up all elements Atoms of the same element are identical Compounds are WHOLE NUMBER ratios of atoms Chemical reactions are when compounds are broken and reformed
36
"Plum Pudding Model" - Thomson (1897)
Immobile electrons
37
Cathode Ray Tube Experiment
Discovered the electron, and they were negative
38
"Atomic Model" - Rutherford (1911)
Nucleus contained protons and neutrons Electrons moved outside of the nucleus
39
Gold Foil Experiment
Discovered the atom was mostly negative space Discovered the positive, small nucleus in the center
40
"Planetary Model" - Bohr (1913)
The nucleus is positively charged Electrons were located in shells (fixed orbits) Electrons can move to other shells
41
Millikin's Oil Drop Experiment (1916)
Oil drop experiment discovered the weight of an electron and the exact charge of an electron
42
Schrodinger (1926)
Electron cloud of probability Heisenberg Uncertainty Principle (either the position OR the speed can be known about an electron, NOT BOTH) Cat thought experiment (electrons move so fast they are everywhere in the cloud at once but also nowhere at any one time)
43
Chadwick (1932)
Discovered the neutron with Rutherford
44
The Atom
There are 2 regions in an atom: the nucleus, and the electron cloud There are 3 parts in an atom: protons, neutrons, and electrons
45
Nucleus
Dense Positively charged Center Small
46
Electron Cloud
Empty space Negatively charged Majority of volume Outside the atom
47
Protons
Located in the nucleus Positively charged Has mass
48
Neutrons
Located in the nucleus No charge Has mass
49
Electrons
Located in the electron cloud (outside of the atom) Negatively charged No mass
50
How to read the periodic table
Top # = Atomic # Middle Letter(s) = Elemental Symbol (Ex. Cu, N) Word = Elemental name Bottom # = Average atomic mass
51
Atomic Number
Number of protons in the nucleus
52
Average Atomic Mass
Average based on percent occurrence of the mass numbers of isotopes
53
Ions
Same element with different electrons from neutral
54
Cation
Positive ion Electrons are LESS than protons
55
Anion
Negative ion Electrons are MORE than protons
56
Isotopes
Same element with different mass numbers from each other Different number of neutrons Ex. Sulfur -32 = 95.002%, Sulfur -33 = 0.76%
57
Calculating Average Atomic Mass
1. Make sure all percentages are in decimal form (58.8% --> 0.588) 2. Multiply the mass of each isotope by the decimal 3. Add the products
58
Radioactivity
Decomposition of the nucleus (nuclear change) All elements above #83 are normally radioactive Becquerel discovered radioactive decay
59
Radioisotopes
Isotopes that are radioactive Ex. Carbon -14
60
Fission
Splitting of an atom's nucleus (occurs naturally on Earth) Ex. Nuclear reactors, nuclear bombs
61
Fusion
2 small nuclei coming together to make 1 nucleus Ex. Celestial stars (like the sun)
62
Half Life
Time it takes for the mass of a radioactive material to decay by half

Chemistry (13 decks)

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