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Chemistry > Matter > Flashcards

Matter Flashcards

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
Q

Phase Changes - Condensation

A

Gas —–> Liquid

26
Q

Phase Changes - Sublimation

A

Solid —–> Gas

27
Q

Phase Changes - Deposition

A

Gas —–> Solid

28
Q

Endothermic

A

A phase change that absorbs heat
Ex. Melting, evaporating, sublimation

29
Q

Exothermic

A

A phase change that releases heat
Ex. Freezing, condensation, deposition

30
Q

Physical Change

A

Does NOT change the chemical composition (chemical formula)
Ex. Phase changes, dissolving, separation of mixtures

31
Q

Seperation - Filtration

A

Separates a mixture by the size of the particles

32
Q

Seperation - Distillation

A

Separates a mixture by boiling points

33
Q

Chemical Change

A

AKA reactions
Chemical bonds are broken and reformed into new compounds
Can be written as an equation
Ex. H2 + O2 —> H2O

34
Q

Signs of a chemical change

A

Change of color
Effervescent (forms a gas)
Forms a precipitate (a solid that can not dissolve)
Temperature change

35
Q

“Billiard Ball Model” - Dalton’s Atomic Theory (1803)

A

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
Q

“Plum Pudding Model” - Thomson (1897)

A

Immobile electrons

37
Q

Cathode Ray Tube Experiment

A

Discovered the electron, and they were negative

38
Q

“Atomic Model” - Rutherford (1911)

A

Nucleus contained protons and neutrons
Electrons moved outside of the nucleus

39
Q

Gold Foil Experiment

A

Discovered the atom was mostly negative space
Discovered the positive, small nucleus in the center

40
Q

“Planetary Model” - Bohr (1913)

A

The nucleus is positively charged
Electrons were located in shells (fixed orbits)
Electrons can move to other shells

41
Q

Millikin’s Oil Drop Experiment (1916)

A

Oil drop experiment discovered the weight of an electron and the exact charge of an electron

42
Q

Schrodinger (1926)

A

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
Q

Chadwick (1932)

A

Discovered the neutron with Rutherford

44
Q

The Atom

A

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
Q

Nucleus

A

Dense
Positively charged
Center
Small

46
Q

Electron Cloud

A

Empty space
Negatively charged
Majority of volume
Outside the atom

47
Q

Protons

A

Located in the nucleus
Positively charged
Has mass

48
Q

Neutrons

A

Located in the nucleus
No charge
Has mass

49
Q

Electrons

A

Located in the electron cloud (outside of the atom)
Negatively charged
No mass

50
Q

How to read the periodic table

A

Top # = Atomic #
Middle Letter(s) = Elemental Symbol (Ex. Cu, N)
Word = Elemental name
Bottom # = Average atomic mass

51
Q

Atomic Number

A

Number of protons in the nucleus

52
Q

Average Atomic Mass

A

Average based on percent occurrence of the mass numbers of isotopes

53
Q

Ions

A

Same element with different electrons from neutral

54
Q

Cation

A

Positive ion
Electrons are LESS than protons

55
Q

Anion

A

Negative ion
Electrons are MORE than protons

56
Q

Isotopes

A

Same element with different mass numbers from each other
Different number of neutrons
Ex. Sulfur -32 = 95.002%, Sulfur -33 = 0.76%

57
Q

Calculating Average Atomic Mass

A
  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
Q

Radioactivity

A

Decomposition of the nucleus (nuclear change)
All elements above #83 are normally radioactive
Becquerel discovered radioactive decay

59
Q

Radioisotopes

A

Isotopes that are radioactive
Ex. Carbon -14

60
Q

Fission

A

Splitting of an atom’s nucleus (occurs naturally on Earth)
Ex. Nuclear reactors, nuclear bombs

61
Q

Fusion

A

2 small nuclei coming together to make 1 nucleus
Ex. Celestial stars (like the sun)

62
Q

Half Life

A

Time it takes for the mass of a radioactive material to decay by half

Chemistry (13 decks)

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