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General Chemistry > Matter > Flashcards

Matter Flashcards

(84 cards)

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1
Q

Is anything that occupies space and has mass

A

Matter

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2
Q

May appear to be continuous and unbroken (but actually discontinuous; since it is made up of tiny particles)

A

Matter

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3
Q

Can be classified based on the physical state, or based on the chemical state or composition

A

Matter

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4
Q

A particular kind of matter that has a fixed composition and distinct properties

A

Pure substance

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5
Q

Matter that contains two or more substances in variable amounts

A

Mixture

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6
Q

a fundamental or elementary substance that cannot be broken down into simpler substances by chemical means.

A

Element

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7
Q

a distinct substance that contains two or more elements combined in a definite proportion by weight.

A

Compound

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8
Q

a water molecule is consists of __?

A

2 H and 1 O atom

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9
Q

Compounds can be classified as:

A

Ionic and Molecular

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10
Q

A type of compound that is held together by attractive forces between their positive and negative charges.

A

Ionic compounds

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11
Q

A type of compound that is held together by covalent bonds

A

Molecular compounds

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12
Q

True or False:

Water does not contain free hydrogen (H₂) or free oxygen (O₂).

A

True

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13
Q

The H₂ part of H₂O means that 2 atoms of hydrogen are combined with one atom of oxygen in the water molecule.

A

Water

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14
Q

A type of mixture that consists of two or more substances, but has one phase of uniform appearance and properties all throughout.

A

Homogenous mixture

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15
Q

a type of mixture with two or more physically distinct phases present

A

Heterogeneous mixture

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16
Q

solute + solvent = solution

A

Homogeneous mixture

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17
Q

The ____ is scattering of light by particles in a color or suspension.

A

Tyndall Effect

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18
Q

what are the physical states of matter?

A

solid, liquid, gas, plasma

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19
Q

the molecules that make up a solid are arranged in regular, repeating patterns. They are held firmly in place but can vibrate within a limited area.

A

Solid

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20
Q

the molecules that make up a liquid flow easily around one another. They are kept from flying apart by attractive forces between them.

A

Liquid

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21
Q

The molecules that make up a gas fly in all directions at great speeds. They are so far apart that the attractive forces between them are insignificant

A

Gas

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22
Q

At the very high temperature of stars, atoms lose their electrons. The mixture of electrons and nuclei that results is the plasma state of matter.

A

Plasma

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23
Q

What’s the 5th state of matter?

A

Bose-Einstein Condensate

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24
Q

It is a gas that is so close to absolute zero that it begins to display quantum effects on a larger scale.

A

Bose-Einstein

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25
Bose-Einstein condensates weren’t created in the laboratory until the (yr)s
1990s
26
- Group of atoms code within absolute zero - Atoms are hardly moving relative to each other— Have almost no free energy to do so, so the atoms begin to clump together and enter the same energy states. They become identical, from a physical point of view, and the whole group starts behaving as though it's a single atom.
Bose-Einstein Condensate
27
True or False: | Mixtures can be created separated by physical means
True
28
True or False: | Compounds can only separated by chemical means
True
29
True or False: Element are pure substances When the subatomic particles of an element are separated from its atom, it no longer retains the properties of that element.
True
30
characteristic of a substance
Property
31
Are attributes that do not depend on the amount of matter
Intensive properties
32
Exist at molecular level, inherent to chemical composition
Intensive properties
33
The property is unchanged by altering the sample size
Intensive properties
34
Or attribute that depend on the amount of matter
Extensive properties
35
Constantly changing attributes, thus cannot be used for identification of certain object or matter
Extensive properties
36
A small matter is added to a system, both mass and volume changes
Extensive properties
37
True or False: While extensive properties are great for describing a sample, they aren’t very helpful in identifying samples because they can change according to sample size because they can change according to sample size or conditions.
True
38
True or False: All chemical properties are intensive. None is extensive. But not all intensive properties are ___
Because chemical properties never depend on how much of a substance is present, but only on what kind of particles make up the substance. Solubility is an intensive property but not a chemical property
39
are observed when a material undergoes chemical change. Nuclear/atomic stability, combustibility, ionization, and relative activity to other substances.
Chemical properties
40
can be observed without changing the composition of the substance.
Physical properties
41
reversible by physical means
Physical change
42
one substance is dissolved in another substance — one substance is dissolved in another substance
The Solution process
43
Changes of Matter
Physical and Chemical
44
a substance goes from one phase to another; solid, liquid, or gas by the addition or removal of heat.
Phase change
45
True or False: | All changes of state are called physical changes because atoms and molecules within do not change.
True
46
True or False: | All physical changes are easily reversible. The original state can be achieved by reversing the change.
True
47
True or False: | The nature of the atoms and molecules involved in a physical change is not altered — chemically they are the same.
True
48
True or False: A few physical changes, like dissolving certain solutes, may result in a temperature change, but most physical changes do not have an energy change associated with them.
True
49
A substance undergoes a reaction and forms products having different properties than the reactants
Chemical change
50
Occurs when the substance’s composition is changed
Chemical change
51
chemical reaction that involves absorption of heat by the system from the surrounding.
Endothermic
52
chemical reaction which involves release of heat by the system to the surrounding
Exothermic
53
Occurs when the nuclei of atoms are rearranged to form new atoms
Nuclear change
54
Involves changes in nuclear structure
Nuclear change
55
- All chemical changes are difficult to reverse. They occur as a result of a reaction between reactant chemicals to make new products. - Reaction can be summarized by chemical equation
Indicators of Change
56
when colorless acid and alkali are mixed, a colorless solution remains. If an indicator is added, there is a color change.
Subtle color change
57
- exothermic process | - increase in temperature
Energy is released
58
- endothermic process | - temperature decreases
Energy is taken in
59
when colorless acid and alkali are mixed, a colorless solution remains. If an indicator is added, there is a color change.
Phase changes
60
the settling of particles or sediment onto a surface. The particles may originate from a vapor, solution, suspension, or mixture.
Deposition
61
the ionization of particles in the upper atmosphere to form the aurora. Ionization may be observed inside a plasma ball novelty toy. Ionization energy required to remove an electron from a gaseous atom or ion.
Ionization
62
a given compound always contains exactly the same proportion of elements by weight. When atoms combine to form compounds, it always has a fixed proportion.
Law of Definite Composition
63
when 2 elements form a series of compounds, the rations of the masses of the second element that combined with one gram of the first element can always be reduced to small whole numbers.
Law of Multiple Proportion
64
no change is observed in the total mass of the substances involved in a chemical change. In a chemical reaction the total mass of the product is equal to the total mass of the reactant.
Law of Conversation Mass
65
energy can be neither created nor destroyed, though it can be transformed from one form of energy to another form of energy.
Law of Conservation of Energy
66
Forms of Energy
Chemical Radiant Mechanical Electrical
67
Types of Energy
Potential | Kinetic
68
energy due to position
potential energy
69
the energy in motion
kinetic energy
70
a source of chemical potential energy
gasoline
71
contains atoms of different elements chemically combined together in a fixed ratio
compound
72
Chemical composition: contains different elements in a fixed ratio arranged in a defined manner through chemical bonds; contains only 1 type of molecule
Compound's chemical composition
73
Mass ratio: has specific mass ratio: pyrite has 46.6% iron and 53.4% sulfur by mass. This is true of all pyrite no matter the sample size
Compound's mass ratio
74
Representation: has chemical formula
Compound's representation
75
Method of Separation: through chemical reaction that breaks the atomic binding the molecules of a compound
Compound's method of separation
76
combination of 2 or more substances that are physically mixed only, no chemical reaction when mixed
Mixture
77
Chemical composition: contains two or more types of pure substances which do not form chemical bonds, visibly distinct components oftentimes
Mixture's chemical composition
78
Mass ratio: has variable mass ratio depending upon what quantities of the ingredients have been combined in the mixture
Mixture's mass ratio
79
Representation: no chemical formula
Mixture's representation
80
Method of separation: physical means: sedimentation or decantation, evaporation, distillation, centrifugation, filtration
Mixture's method of separation
81
Molecules composed of two or more elements
Molecular compound
82
Cations with positive charge; anions with negative charge
Ionic compound
83
measure of how easily a material is scratched
Hardness
84
ability to be stretched/drawn into fine wires
Ductility

General Chemistry (6 decks)

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