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NC Earth & Environmental Science > Chemistry and Matter > Flashcards

Chemistry and Matter Flashcards

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1
Q

Extensive

A

Describes matter depending on the amount of matter in the sample.

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2
Q

Intensive

A

Describes matter depending on the type of matter, the contents (not the amount).

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3
Q

Physical Properties

A

A property which can be observed and measured without changing the material’s composition

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4
Q

Chemical Properties

A
  • A property which can be observed by changing the composition of the material (after a chemical reaction)
  • The ability to undergo a specific chemical change
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5
Q

Plasma

A

Formed at high temperatures; ionized phase of matter

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6
Q

Mixtures

A

A physical blend of two or more substances which have variable composition

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7
Q

Heterogenous Mixture

A

A mixture which is not uniform in composition (ex. chocolate-chip cookie)

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8
Q

Homogenous Mixtures

A

Same composition throughout; called “solutions” (powder-drinks, air)

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9
Q

Solutions

A
  • Homogeneous Mixture
  • Includes a ‘solute’ and ‘solvent’
  • Mixed by molecule to molecule, and can occur between any state of matter
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10
Q

Phase

A

Any part of a sample with uniform composition of properties

ex. Homogeneous mixture consists of a phase, heterogeneous consists of 2+ phases

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11
Q

Separating Mixtures:

A

Differences in properties can be used to separate mixtures

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12
Q

Elements

A

Simplest kind of matter; cannot be broken down to have the same properties!
(One kind of matter)

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13
Q

Compounds

A
  • Substances which can only be broken down by chemical methods
  • Made of 2+ atoms that are chemically combined
  • Will have completely different properties if broken down
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14
Q

Chemical Change

A

A change in which one or more substances is converted into new substances with change to composition.
Signs of a chemical change include heat and light.

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15
Q

Precipitate

A

A solid that separates from solution (won’t dissolve)

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16
Q

Signs of Chemical Change:

A
  • Energy is absorbed or released (temp.)
  • Color changes
  • Gas production
  • Precipitate
  • Irreversibility
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17
Q

Law of Conservation of Mass

A

During any chemical reaction, the mass of the products is always equal to the mass of the reactants.

18
Q

Symbols and Formulas:

A

Elements are represented by a 1 or 2 letter symbol; compounds are represented by a formula.
(ex. He = Helium; H20 = Water)

19
Q

Atomic Number

A

The number of protons in an atom (in the nucleus)!

Elements are different because they have different amounts of protons.

20
Q

Overall Charge:

A

All elements in nature have a neutral overall charge, therefore the number of protons equals the number of electrons.

21
Q

Mass Number

A

The number of protons and neutrons in the nucleus of an isotope. (Rounded atomic mass)

22
Q

Isotope

A

Element can vary based on the number of neutrons (and still be the same element).

23
Q

Electron Mass:

A

9.11 x 10^-28

Much less mass than protons and Neutrons

24
Q

Proton or Neutron Mass

A

1.67 x 10^-24

Majority of the Mass is in the Nucleus

25
Q

Periodic Law

A

When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

26
Q

3 classes of Elements

A
  1. Metals - Electrical conductors, have luster, ductile, malleable (can be shaped or drawn out)
  2. Non-Metals - Generally brittle and non-lustrous, poor conductors of heat and electricity (hard, but can snap or break)
  3. Metalloids - Properties are intermediate between metals and nonmetals.
27
Q

Group of Elements

A

Group 1A - Alkali metals (very reactive; forms a base with water)

Group 2A - Alkaline Earth metals (do not dissolve well; reactive; Earth metals and also form base with water)

Group 7A - Halogens (wants one more electron)

Group 8A - Noble gases (stable and don’t react due to a full shell of electrons)

28
Q

Solute

A

Something which dissolves in the solvent (usually liquid) to make a solution.

29
Q

Solvent

A

Usually a liquid, does the dissolving of a solute to make a solution

30
Q

3 Classes of Mixtures

A
  • Solutions
  • Colloid
  • Suspension
31
Q

Solution:

  1. Ex.
  2. Particle Type:
  3. Particle Size:
  4. Scatter Light?
  5. Settle while standing?
  6. ​Separate by filtration?
A

Always transparent, so that particles do not have to scatter light.

  1. Ex. - Salt water, air
  2. Particle Type - Ions, atoms
  3. Particle Size - Small
  4. Scatter Light? - No
  5. Settle while standing? - No
  6. ​Separate by filtration? - No
32
Q

Colloid:

  1. Ex.
  2. Particle Type:
  3. Particle Size:
  4. Scatter Light?
  5. Settle while standing?
  6. ​Separate by filtration?
A

A mixture where one of the substances is split into small particles that are dispersed throughout another substance. The small particles are called colloidal particles.

  1. Ex. - Soot, fog
  2. Particle Type - Small clusters
  3. Particle Size - Medium
  4. Scatter Light? - Yes
  5. Settle while standing? - No
  6. ​Separate by filtration? - No
33
Q

Suspension:

  1. Ex.
  2. Particle Type:
  3. Particle Size:
  4. Scatter Light?
  5. Settle while standing?
  6. ​Separate by filtration?
A

A heterogeneous mixture in which the solute particles do not dissolve in a liquid, and instead spread throughout the liquid.

  1. Ex. - Muddy water, Flour, Paint, Chalk in water, etc…
  2. Particle Type - Large clusters
  3. Particle Size - Large
  4. Scatter Light? - Yes
  5. Settle while standing? - Yes
  6. ​Separate by filtration? - Yes
34
Q

Tyndall Effect

A

Light passes through a colloid or suspension (particles scatter light).

35
Q

Emulsion

A

A mixture where two or more liquids are unblendable (such as oil and water), causing a liquid-liquid separation.

36
Q

Periodic Table:

A

Displays the symbols and names of the elements, along with information about the structure of their atoms. (Atomic Number and mass)

37
Q

Balanced Chemical Equation

A
  • Atoms cannot be created or destroyed
  • Same number of elements on both sides of the equation

Ex. 2_Na + 2_H2O –> _H2 + 2_NaOH

38
Q

The Skeleton Equation

A

A chemical equation which does not indicate how many elements; meaning NOT balanced.

Ex. _Na + _H2O –> _H2 + _NaOH (Notice the Coefficients are missing)

39
Q

” (aq) “ - after the chemical formula

A

Dissolved in water, an aqueous solution: NaCl (aq) is a salt water solution

40
Q

arrow points up - after the chemical formula

A

Used after a product showing that a gas has been produced.

41
Q

arrow points down - after the chemical formula

A

Used after a product indicating a solid has been produced

42
Q

Rules of Balance (Chemical Equations):

A
  • Assemble the correct formulas for all the reactants and products, using “+” and “–>”
  • Count the number of atoms of each type appearing on both sides
  • Balance the elements on at a time by adding coefficients (the numbers in front) where you need more – save balancing H and O until LAST! (Oxygen is last)
  • Coefficient must be in the front!
  • Subscript cannot be changed, only coefficients, or it becomes a different compound.

NC Earth & Environmental Science (9 decks)

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