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Chemistry Lecture EN 1-23s > Reviewer Midterms > Flashcards

Reviewer Midterms Flashcards

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1
Q

This branch focuses on the study of carbon-containing compounds, duding their structure, properties, synthesis, and reactions. Organic chemistry is crucial in areas such as pharmaceuticals, polymers, dyes, and many natural products Inorganic Chemistry Inorganic chemistry deals with the study of elements and their compounds.

A

Organic Chemistry.

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2
Q

excluding carbon-based compounds. It covers topics like metals, minerals, nonmetals. ordination compounds, and materials chemistry. Phys Chemistry: Physical chemistry combines principles of physics and chemistry to untend the fundamental properties and behavior of matter. It encompasses topics such as Temodynamics, quantum mechanics, spectroscopy, kinetics, and electrochemistry

A

Inorganic chemistry

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3
Q

methods to determine the composition, structure, and concentration of substances.

A

Analytical chemistry

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4
Q

explores the chemical processes and substances that occur within living organisms. It investigates topics such as proteins, enzymes, DNA, metabolism, and the blochemical basis of diseases.

A

Biochemistry

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5
Q

studies the impact of chemicals on the environment and how natural processes affect the distribution and behavior of chemical species

A

Environmental chemistry

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6
Q

focuses on the synthesis, characterization, and design of new materials with desired properties for various applications, including electronics, energy storage, catalysis, and nanotechnology.

A

Materials chemistry

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7
Q

employs computational methods and mathematical models to understand and predict the behavior of chemical systems. It contributes to the interpretation of experimental data and the development of new theories.

A

Theorical Chemistry

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8
Q

involves the application of chemical principles to large- scale production processes. It plays a crucial role in sectors like pharmaceuticals, petrochemicals, polymers, fertilizers, and consumer goods.

A

Industrial chemistry

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9
Q

combines knowledge from various fields to design and develop drugs. It involves the synthesis, characterization, and optimization of chemical compounds for therapeutic purposes.

A

Medicinal chemistry

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10
Q

anything that occupies space and has mass. It is one of the fundamental concepts in Physics and Chemistry, and it is all around us in the form of solids, liquids, gases and plasma Matter can exist in different states depending on the condition of temperature and pressure.

A

Matter

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11
Q

is the “stuff” of the universe: air, glass, planets, students- anything that has mass and volume.

A

Matter

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12
Q

the types and amounts of simpler substances that make it up.

A

Composition

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13
Q

is a type of matter that has defined, fixed composition.

A

Substance

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14
Q

the characteristics that give each substance its unique identity

A

Properties

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15
Q

Are those that a substance shows by itself, without changing into or interacting with another substance.

A

Physical properties

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16
Q

are those that a substance shows as it changes into or interacts with another substance (or substances

A

Chemical properties

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17
Q

Three states of matter

A

Solid
Liquid
Gas

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18
Q

Depends on the quantity of matter observed

A

Extensive property

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19
Q

Is dependent of the amount of matter observed.

A

Intensive property

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20
Q

Is a function of temperature because volume varies with temperature, whereas mass remains constant.

A

Density

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21
Q

Matter is made up of very tiny units called?

A

Atoms

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22
Q

Is a substance made up of only a single type of atoms

A

Chemical element

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23
Q

Are substances in which atoms of two or more different elements are combined with one another

A

Chemical compound

24
Q

Is the smallest entity having the propositions of the constituent atoms as does the compound as a whole

A

Molecule

25
Q

can be separated into pure substances by physical methods. Pure substance is one with constant composition.

A

Mixtures

26
Q

are uniform in composition and properties throughout a given sample but variable from one sample to another.

A

Homogeneous mixture

27
Q

the components separate into distinct regions

A

Heterogeneous mixture

28
Q

The scientific system of measurement is called?

A

Systeme internationale d’ unites

29
Q

is the comparison of a physical quantity to be measured with a unit of measurement-that is with a fixed standard of measurement

A

Measurement

30
Q

are those aspects in the universe that can be measured by any desired unit of measurement.

A

Physical quantity

31
Q

describes the quantity of matter in an object.

A

Mass

32
Q

is the degree of hotness and coldness, but necessarily a measure of heat. It is a measure of the average kinetic energy of molecules of a substance.

A

Temperature

33
Q

A property of matter that is often used by chemists as an “identification tag” for a substance is

A

Density

34
Q

a French chemist who ultimately elucidated the true nature of combustion, thus clearing the way for the remarkable development that was made near the end of eighteenth century.

A

Antoine Lavoisier

35
Q

Mass is neither created nor destroyed

A

La of conservation of mass

36
Q

A given compound always contains exactly the same proportion of elements by mass

A

Low of definite proportion

37
Q

When two elements form a series d compounds, the ratios of the masses of the second elements that combine with 1 gramd the first element can always be reduced to small whole numbers.

A

Law of multiple proportion

38
Q

Each element is made up of tiny particles called storms

A

Dalton’s atomic theory

39
Q

an English schoolteacher, the Greek atomist held the theory of the structureless atom (also known as the Billiard Ball model). There were only gut feelings and no experimental data

A

John Dalton

40
Q

The raisin bread model, sometimes known as the plum pudding model, was put out by English physicist

A

Jj Thomson

41
Q

came up with the Prout’s Model. The atomic masses of the known elements were integral multiples of hydrogen’s atomic mass, which served as the foundation for his model.

A

William prout

42
Q

Nuclear model proposed by _____, British physicist was considered another model of atoms. The basis of this model was the observations from the alpha particle scattering experiments done with Hans Geiger, Rutherford’s German assistant.

A

Ernest Rutherford

43
Q

An additional idea regarding an atom was the solar system model put forth by. Emest Rutherford served as the inspiration for this concept, and Niels Bohr put the electrons in orbits.

A

Neils Bohr

44
Q

German physicist ______, who lived from 1887 to 1961, proposed the quantum mechanical model, sometimes known as the wave model. This atom model was based on the dual duality of light and matter.

A

Erwin Schroedinger

45
Q

Principle states that the orbitals are filled in order of increasing energy. A mnemonic device has been developed to enable one to determine the order of increasing energy of the orbital and therefore the order of filling of the orbital.

A

Aufbau principle

46
Q

rule specifies that orbital should be filled singly before pairing.

A

Hund’s rules of maximum multiplicity

47
Q

Principle specifies that the maximum number of electrons which an orbital may accommodate is two. This arise from the requirement that no two electrons in an atom can have all for quantum numbers identical at least one must be different.

A

Puli exclusion principle

48
Q

who in 1864 suggested that elements should be arranged in octaves, based on the idea that certain properties seemed to repeat for every eight elements in a way similar to the musical scale which repeats for every eight tone.

A

John newlands

49
Q

The present form of the periodic table was conceived independently by two chemists: The German ______ and russian ______

A

Julius lothar meyer and Dmitri ivanovich Mendeleev

50
Q

states that the properties of elements are functions of their atomic numbers. There is no single best form to represent the periodic table. The

A

Modern periodic table law

51
Q

are the electrons that occupy the outermost main energy level of the atom in the ground state

A

Valence electron

52
Q

Electrons in inner main energy levels are called

A

Core electrons

53
Q

is the average size of the atom when it has lost or gained electrons. A loss of electron or cation formation results in a decrease in radius. A gain of electrons or anion formation results in an increase in radius.

A

Ionic radious

54
Q

Is the energy required to remove an electron from an atom

A

Inonization energy

55
Q

is the negative of electron gain enthalpy. If defined in this way, the trend given above is true: the more positive the value of electron affinity, the tendency of the atom to gain electrons is great

A

Electron affinity

56
Q

is the ability of an atom to attract shared electrons. It is expressed as ; numerical value that was calculated from other measurable properties.

A

Electronegativity

57
Q

are substances having the same number of electrons

A

Isoelectronic substance

Chemistry Lecture EN 1-23s (1 decks)

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