Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Science 311 Test > Physical Science: Chemistry > Flashcards

Physical Science: Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
Biology 101 flashcards
1
Q

Solid Sphere Model

A

Dalton’s model of the atom as solid and indivisible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Atoms

A

the smallest unit of an element that has properties of that element

carbon atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Solute

A

The material in a solution that is dissolved in the solvent

The sugar in lemonade

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Molarity (M)

A

the concentration of a solute per liter of solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Solution

A

a mixture in which one substance dissolves in another

simple syrup (sugar and water)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Heterogeneous Mixture

A

a mixture that is not uniformly mixed

granola with raisins at the bottom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Saturated

A

A solution that cannot dissolve any more solute

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Neutron

A

neutral particle found in the nucleus of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Compound

A

groups of two or more different elements held together by ionic or molecular bonds

NaCl and H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Proton

A

positively charged particle found in the nucleus of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Solvent

A

a substance which dissolves other substances

if salt is dissolved in water, water is the solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Nuclear Model

A

Rutherford discovered the nucleus and that protons were located here

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Electron

A

low-mass, negatively charged particle; surrounds the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Quantum Model

A

Schrodinger theorized that the electrons move in clouds around the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Supersaturated

A

A solution that was saturated and when heated has the ability to dissolve more solute and then it is cooled rapidly

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Concentrated

A

Contains more solute than a diluted solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Pure Substance

A

a substance that consists of only one type of atom or molecule

helium gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Diluted

A

Contains less solute than a concentrated solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Planetary Model

A

Bohr identified that electrons orbited the nucleus in a fixed orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Nucleus (of the Atom)

A

the positively charged, small, central core of an atom; made of protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Plum Pudding Model

A

Created by JJ Thompson, the protons, neutrons and electrons floated around the atom like fruit in a pudding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Unsaturated

A

A solution that has the ability to dissolve more solute

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Emission Spectrum

A

A series of colored lines of different wavelengths (or frequencies) produced when electrons in atoms fall from higher to lower energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Ground State

A

the lowest-energy arrangement of electrons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Element

A

an atom with a unique number of protons in its nucleus

iron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Mixture

A

a substance in which the atoms, molecules, or particles of two or more different materials are mixed but not chemically combined

salad

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Homogeneous Mixture

A

a mixture with the same ratio of parts throughout the mixture

salt dissolved in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Photoelectric Effect

A

Electrons are ejected from a metal when illuminated with light at a high enough frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Entanglement

A

Entangled particles instantly share information with each other even when separated by a great distance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Matter

A

anything that has mass and takes up space

mud

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Metallic Bond

A

A bond between 2 metal atoms that occurs when electrons are released into the shared area and the atoms are attracted to the space.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Percent Composition

A

The atomic mass of the desired element divided by the total atomic mass of the molecule and multiplied by 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Triple Bond

A

An atomic bond between atoms that share three pairs of electrons

N ≡ N

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Cation

A

A positively charged atom that has given up an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Avogadro’s Number

A

the number of atoms in 1 mole of carbon-12.

36
Q

Double Bond

A

An atomic bond between atoms that share two pairs of electrons

C = O

37
Q

Empirical Formula

A

Shows the ratio of atoms in a molecule, not the actual number of molecules.

38
Q

Chemical Formula

A

written expressions of a molecule; tells the number of atoms of each type of element in one molecule

39
Q

Moles of Atoms

A

The atomic mass of the molecule divided by Avogadro’s number

40
Q

Anion

A

A negatively charged atom that has gained an electron

41
Q

Polar Bond

A

A bond between 2 atoms in which one has a slightly stronger pull on the shared electron resulting in oppositely charged poles

42
Q

Polyatomic Ions

A

Molecules with a non-zero charge that form from more than one atom

OH-

43
Q

Ionic Bond

A

a chemical bond between oppositely charged atoms when electrons are removed from one atom and given to an atom of another element

salt (NaCl)

44
Q

Electron Dot

A

Shows only the number of valence electrons in an atom.

45
Q

Molecular Bond / Covalent Bond

A

a chemical bond formed when two atoms share their outer electrons; formed between two nonmetal atoms

bond between carbon and oxygen (CO2)

46
Q

Hydrogen Bond

A

a weak attraction between hydrogen and some other element in another compound

hydrogen bonds attach water molecules to other water molecules

47
Q

Molecular Formula

A

Shows the actual number of atoms, not the ratio as in the empirical formula.

water is H₂O which means there are 2 hydrogen atoms and 1 oxygen atom in each atom

48
Q

Pauling Units (PU)

A

measures the electronegativity of a bond

49
Q

Single Bond

A

An atomic bond between atoms that share one pair of electrons

C - C

50
Q

Nonpolar Bond

A

A bond between 2 atoms of the same element that equally pull on the shared electron

51
Q

Standard Temperature and Pressure (STP)

A

A temperature and pressure of 273 K and 1 atm

52
Q

Limiting Reagent / Limiting Reactant

A

The first chemical to be used up in a chemical reaction

53
Q

Dynamic Chemical Equilibrium

A

Equilibrium when a reversible reaction proceeds in both directions, so the net production is zero

54
Q

Chemical Reaction

A

a reaction that forms a new substance by rearranging the atomic bonds between atoms. The process absorbs energy during bond-breaking and releases energy during bond-making.

HCl+NaOH→NaCl+H2O

55
Q

Chemical Equilibrium

A

The state in which reactants and products are being formed at the same rate

56
Q

Le Chatelier’s Principle

A

The statement that a reaction shifts to counteract a change in concentration or temperature of the reactants

If the pressure on a reaction at equilibrium is increased, then the reaction will shift to produce fewer moles of gas.

57
Q

Conservation of Matter

A

Matter cannot be created or destroyed; it only changes form

chemical reaction

58
Q

Reaction: Combination

A

2 elements or molecules combine to form 1 molecule

A+B -> AB C +O2 –> CO2

59
Q

Excess Reagent / Excess Reactant

A

The leftover reagent(s) in a chemical reaction after the limiting reagent is depleted.

60
Q

Endothermic

A

In an endothermic process, a substance gains thermal energy.

In an endothermic reaction, the reactants absorb heat while rearranging chemical bonds.

As ice melts into water, it absorbs heat from the environment

61
Q

Exothermic

A

In an exothermic process, a substance releases thermal energy.

In an exothermic reaction, the reactants release heat while rearranging chemical bonds.

As water freezes into ice, it releases heat into the environment

62
Q

Stoichiometry

A

uses a balanced chemical equation to determine the amount of reactants needed to create a certain amount of product or how much product can be created from a set amount of reactant

63
Q

Reaction: Double Replacement

A

Elements in molecules replace each other

64
Q

Reaction: Single Replacement

A

One element or molecule replaces another element in a molecule

65
Q

Reaction: Decomposition

A

1 molecule is broken down into 2 separate elements or molecules

66
Q

Pressure

A

the force exerted on an object over a given area

67
Q

Reaction: Oxidation/Reduction (Redox)

A

Reaction in which electrons transfer, causing the oxidation number to change

68
Q

Static Chemical Equilibrium

A

Equilibrium reached in an irreversible reaction that proceeds in one direction until all the reactants are used up

69
Q

Oxidation Number

A

The charge on an atom

70
Q

Activation Energy (Ea)

A

The amount of energy needed for a reaction to begin

71
Q

Reaction: Neutralization

A

Reaction in which when an acid and base chemically react and form a salt and water with a resulting pH of 7

72
Q

Reaction: Combustion

A

A compound containing carbon reacts with oxygen and burns releasing carbon dioxide

73
Q

Chemical Equations

A

Notation that shows how 2 molecules or compounds react together to form a product

74
Q

Gibbs Free Energy (ΔG)

A

The change in enthalpy minus the product of temperature and the change in entropy, measured in kJ per mol reaction

75
Q

Spontaneity

A

Whether or not a process will proceed without an additional energy input;
ΔG<0

76
Q

Solubility

A

the ability of a substance to be dissolved

77
Q

Exothermic

A

In an exothermic process, a substance releases thermal energy.

In an exothermic reaction, the reactants release heat while rearranging chemical bonds.

As water freezes into ice, it releases heat into the environment

78
Q

Solvent

A

a substance which dissolves other substances

if salt is dissolved in water, water is the solvent.

79
Q

Calorimeter

A

A piece of equipment used to determine the heat change associated with a chemical reaction

80
Q

Endothermic

A

In an endothermic process, a substance gains thermal energy.

In an endothermic reaction, the reactants absorb heat while rearranging chemical bonds.

As ice melts into water, it absorbs heat from the environment

81
Q

Specific Heat (c)

A

The heat energy required to raise the temperature of a substance with a given mass by a given number of degrees.

Δheat=mcΔT

82
Q

Standard Gibbs Free Energy of Formation (ΔGfo)

A

The change in energy that results from the formation of 1 mole of chemical from its component elements at 298 K

83
Q

Enthalpy (H)

A

The quantity of heat in a system

84
Q

Entropy (S)

A

A measure of the disorder of a system. The amount of thermal energy that cannot be used to do mechanical work as a system moves toward equilibrium.

85
Q

Enthalpy of Solution / Enthalpy of Dissolution (ΔHsoln)

A

the heat that is absorbed or released when a solute dissolves into solution.

In an exothermic dissolution, the interactions between the solute particles are weaker than the interactions between solute and solvent particles. The ΔHsoln is negative.

In an endothermic dissolution, the interactions between solute particles are stronger than the interactions between solute and solvent particles. The ΔHsoln is positive.

86
Q

Dissolution

A

The separation of an ionic compound into a cation and anion

Breaking apart of ionic NaCl salt crystal in water.

Science 311 Test (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions