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Science Olympiad > It Matters! > Flashcards

It Matters! Flashcards

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0
Q

Liquid

A

A phase of matter. It occurs at a higher temperature than solids and a lower temperature than gases. Liquids take the shape of the container they’re in. They have a fixed volume.

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1
Q

Solid

A

A phase of matter. It occurs at the lowest temperatures and is characterized by a held shape and fixed volume.

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2
Q

Gas

A

A phase of matter. It occurs at higher temperatures than liquids and lower temperatures than plasmas. Gases take the shape of their container and fill up the volume of the container they’re in.

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3
Q

Plasma

A

A phase of matter, which occurs at extremely high temperatures. Similar to a gas, but made up of free electrons and ions of an element: the electrons are stripped from their parent atom.

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4
Q

Structure of the Atom

A

Nucleus in center that contains protons and neutrons. Electrons orbit around atom in probability clouds called orbitals.

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5
Q

Behavior of Atoms in: Solids, Liquids, Gases, Plasmas

A

Solid: atoms are fixed in place
Liquid: atoms can move but are still connected to each other
Gases and Plasmas: Atoms can move freely and independently of each other.

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6
Q

Heterogeneous

A

A combination of substances that do not have uniform composition and properties.

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7
Q

Homogenous

A

A mixture where the components are uniformly distributed.

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8
Q

Elements

A

Atoms. The building blocks of the universe.

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9
Q

Compounds

A

The chemical combination of two or more elements.

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10
Q

Mixtures

A

The non-chemical combination of two or more elements or compounds.

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11
Q

Colloid Mixture

A

A mixture where microscopically dispersed insoluble particles are suspended throughout another substance. Does not settle/takes a very long time to settle.

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12
Q

Suspension Mixture

A

A heterogeneous mixture with solid particles (larger than one μm) dispersed via mechanical agitation. They eventually settle.

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13
Q

Solution Mixture

A

A homogenous mixture consisting of only one phase. A solute is dissolved in a solvent. The concentration is a measure of the amount of solute compared to solvent.

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14
Q

Magnetism

A

A property of matter. When placed in a magnetic field, matter is either paramagnetic (attracted) or diamagnetic (repulsed).

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15
Q

Conductivity

A

A measure of how well a material conducts heat and electricity.

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16
Q

Flexibility

A

The ability of a material to bend without breaking and to return to its original shape or size.

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17
Q

Hardness

A

The ability of a material to withstand scratches.

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18
Q

Ductility

A

The ability of a metal to deform without breaking or fracturing.

19
Q

Malleability

A

The ability of a metal to be hammered, forged, pressed, or rolled into thin sheets.

20
Q

Luster

A

How shiny a substance is

21
Q

Opacity

A

How well a substance can be seen through.

22
Q

Strength

A

The measure of how well a substance handles stresses and strains

23
Q

Viscosity

A

Specific to fluids, a measure of its resistance to deformation by shear or tensile stress (such as gravity)

24
Q

Mass

A

An extensive property, a measure of the amount of matter in an object.

25
Q

Volume

A

An extensive property, the measure of the amount of space an object occupies.

26
Q

Density

A

The mass of a substance divided by its volume.

27
Q

Buoyancy

A

The ability of a substance to float in a liquid, dependent on its density.

28
Q

Freezing

A

The phase transition from liquid to solid.

29
Q

Melting

A

The phase transition from solid to liquid.

30
Q

Condensation

A

The phase transition from gas to liquid.

31
Q

Evaporation

A

The phase transition from liquid to gas.

32
Q

Ionization

A

The phase transition from gas to plasma.

33
Q

Deionization

A

The phase transition from plasma to gas.

34
Q

Sublimation

A

The phase transition from solid to gas.

35
Q

Deposition

A

The phase transition from gas to solid.

36
Q

Physical Change

A

Any (USUALLY BUT NOT ALWAYS) reversible change that occurs without altering the chemical composition of a substance, such as changing color, shape, state of matter, or volume.

37
Q

Chemical Change

A

A (USUALLY BUT NOT ALWAYS) irreversible change in the chemical composition of a substance.

38
Q

Law of Conservation of Mass

A

Matter can be changed from one form into another, but never created nor destroyed.

39
Q

Law of Definite Proportions

A

(Also known as Proust’s Law) A chemical compound always contains exactly the same proportion of elements by mass.

40
Q

Law of Multiple Proportions

A

(Also known as Dalton’s Law) When two elements combine with each other to form two or more compounds, the ratios of the masses of one element that combines with the fixed mass of the other are simple whole numbers.

41
Q

Ionic Bonds

A

Bonds between a metal and a non-metal (the non-metal “donates” one or more electrons to the metal)

42
Q

Covalent Bonds

A

Bonds between nonmetals where electrons are shared.

43
Q

Metallic Bonds

A

Bonding between metals, sharing of a sea of delocalized electrons amongst a lattice of positive ions. The electrons act as a “glue” giving the substance a definite structure.

44
Q

Electronegativity

A

The measure of the tendency of an atom to attract a bonding pair of electrons. The trend goes up and to the right on the table, making Fluorine and Francium the most and least electronegative elements respectively.

45
Q

Enthalpy

A

The amount of heat content used or released in a system at constant pressure.

46
Q

Entropy

A

Degree of disorder in system

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