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GEN CHEM > GEN CHEM PART 1 > Flashcards

GEN CHEM PART 1 Flashcards

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1
Q

It consists of a positively charged core (the atomic nucleus) which contains protons and neutrons, and which maintains a number of electrons to balance the positive charge in the nucleus.

A

Atoms

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2
Q

He proposed an alternate view, referred to as the discontinuous theory of matter.

A

Democritus

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3
Q

He named the building blocks of matter atomos, meaning literally “indivisible,”

A

Democritus

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4
Q

They formulated the notion that there can be no ultimately indivisible particles

A

Plato and Aristotle

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5
Q

Theory that states elements are composed of extremely small particles, called atoms.

A

Dalton’s Atomic Theory

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6
Q

Theory that states atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements.

A

Dalton’s Atomic Theory

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7
Q

Theory that states that compounds are composed of atoms of more than one element. In any compound, the ratio of the numbers of atoms of any two of the elements present is either an integer or a simple fraction.

A

Dalton’s Atomic Theory

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8
Q

A theory that states chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in their creation or destruction.

A

Dalton’s Atomic Theory

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9
Q

Theory that states atoms may be disintegrated.

A

Modern Atomic Theory

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10
Q

In nuclear reactions, atoms are being transferred into atoms of single elements in a process known

A

nuclear transmutation

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11
Q

Theory that states that not all atoms of any given element are alike.

A

Modern Atomic Theory

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12
Q

Theory that states not all atoms of a given element pose identical properties except in mass.

A

Modern Atomic Theory

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13
Q

Theory that states atoms of different elements have different properties.

A

Modern Atomic Theory

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14
Q

Electrons are discovered by

A

Joseph John Thomson

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15
Q

It is the first component of the atom to be identified

A

Electron

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16
Q

Electron mass

A

9.109 x 10-31 kg

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17
Q

Electron charge

A

-1.602 x 10-19 coulombs

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18
Q

One of the components of a nucleus

A

Protons

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19
Q

Protons was discovered by

A

Eugene Goldstein

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20
Q

Protons mass

A

1.673 x 10-27 kg

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21
Q

Neutrons was discovered by

A

James Chadwick

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22
Q

Neutrons mass

A

1.675 x 10-27 kg

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23
Q

His theory stated that atoms are indivisible,those of a given element are identical and compounds are combination of different types of atoms.

A

John Dalton

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24
Q

He discovered corpuscles in atoms. He subsequently produced “plum pudding” model of atom. It shows the atom as composed of electrons scattered throughout a spherical cloud of a positive charge.

A

Joseph John Thomson

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25
Q

He fired positively charged alpha particles at a thin sheets of gold foil. Most passed through with a little deflection but some deflected at large angles.

A

Ernest Rutherford

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26
Q

He modified Rutherfords model of the atom by stating that electrons moved around the nucleus in orbits of fixed size and energies.

A

Niels Bohr

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27
Q

He stated that electrons do not move in set paths around nucleus but in waves. He stated also the ‘cloud of probability’ called orbitals in which more likely to find electrons.

A

Erwin Schrodinger

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28
Q

Model that states that atoms is a spherical mass containing electrons and that this spherical mass is positive but is made neutral by the electrons embedded in it.

A

Thomson Model

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29
Q

It is based on additional experimental evidence of “alpha scattering experiments”.

A

Rutherford model

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30
Q

In this model, protons are in the nucleus and the electrons are in the orbital motion around the nucleus.

A

Bohr Model of an Atom

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31
Q

In this model, the atoms are in elliptical orbits of increasing number.

A

Rutherford-Bohr Model

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32
Q

This principle states that simultaneous determination of the exact position and exact momentum of electron is impossible.

A

Heisenburg Uncertainty Principle

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33
Q

In this model, the nucleus is a single cluster of particles at the center of the atom while the electrons are everywhere

A

Wave Mechanical Atom

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34
Q

This theory makes the assertion that electromagnetic radiation like X-rays, gamma rays, radio waves and light rays are made up of small bits of energy.

A

Schroedinger “Quantum Model”

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35
Q

This theory states that the number of orbital types in a given shell is equal to the shell number.

A

Orbital theory

36
Q

The number of protons in the nucleus of an atom of an element also the number of electrons in an atom

A

Atomic Number

37
Q

It ia total number of protons and neutrons on the nucleus of nucleons

A

Mass Number

38
Q

atoms of the same element with the same atomic number, but different mass numbers.

A

Isotopes

39
Q

They have the same number of protons and electrons but different number of neutrons.

A

Isotopes

40
Q

Atoms of different elements having the same number of neutrons.

A

Isotones

41
Q

Atoms of different elements having the same atomic mass.

A

Isobars

42
Q

It is a charged species, an atom or a molecule, that has lost or gained one or more electrons.

A

Ions

43
Q

It is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances.

A

Molecules

44
Q

It is an electrode of a polarized electrical device through which conventional current enters the device.

A

Anode

45
Q

It is an electrode of the device through which conventional current leaves the device.

A

Cathode

46
Q

Are the physical properties of matter which may vary from time to time.

A

Extrinsic Property

47
Q

Not the characteristics of the substance itself

A

Physical property

48
Q

Depends on the amount, also called extensive properties.

A

Extrinsic Property

49
Q

Are the properties of matter which are constant.

A

Intrinsic Property

50
Q

Give the characteristics of the substance its unique identity.

A

Intrinsic Property

51
Q

Those which do not depend on the amount, also called intensive properties.

A

Intrinsic Property

52
Q

Constant at any place and time

A

Mass

53
Q

A measure of the quantity of matter in an object

A

Mass

54
Q

When travelled to the moon, the mass of an object will still be the same

A

Mass

55
Q

Can never be zero

A

Mass

56
Q

Varies, depends on the amount of gravity

A

Refers to the downward pull of the objects towards the center of the earth; the force that gravity exerts on an object.

57
Q

When travelled to the moon, the weight of an object will only be 1/6 of its weight on earth

A

Weight

58
Q

Can also be zero

A

Weight

59
Q

It is the fundamental materials of which all matter is composed.

A

Element

60
Q

It is any substance composed of identical molecules consisting of atoms of two or more chemical elements

A

Compound

61
Q

It is any of a class of substances characterized by high electrical and thermal conductivity as well as by malleability, ductility, and high reflectivity of light.

A

Metal

62
Q

It lacks metal properties and is capable of forming anions, acid oxides, acids, and stable hydrogen compounds.

A

Non metal

63
Q

It is a chemical element that forms a simple substance having properties intermediate between those of a typical metal and a typical nonmetal.

A

metalloid

64
Q

earth’s crust composition

A

Oxygen, Silicon, Aluminum, Iron, Calcium, Magnesium

65
Q

Human body composition

A

Oxygen, Carbon, Hydrogen, Nitrogen, Calcium, Phosphorus

66
Q

It is a neutral compounds made up of positively charged ions called cations and negatively charged ions called anions

A

Ionic compound

67
Q

It is formed by sharing one or more pairs of valence electrons.

A

Covalent compound

67
Q

It is formed by sharing one or more pairs of valence electrons.

A

Covalent compound

68
Q

It is compound that contains one or more metal elements bonded to another element.

A

Metallic compound

69
Q

It is a homogenous mixture of two or more substances in relative amounts that can be varied continuously up to what is called the limit of solubility.

A

Solutions

70
Q

It is any substance consisting of particles substantially larger than atoms or ordinary molecules but too small to be visible to the unaided eye

A

Colloid

71
Q

It is heterogeneous mixture in which the solid particles are spread throughout the liquid without dissolving in it.

A

Suspension

72
Q

It is stable dispersion of two or more immiscible liquids held in suspension by small percentages of substances called emulsifiers.

A

Emulsion

73
Q

Always have a definite composition by weight.

A

Compound

74
Q

Components may be present in any proportions.

A

Mixture

75
Q

Preparation shows evidence of chemical action taking place.

A

Compound

76
Q

It is prepared with no evidence of any chemical reaction taking place.

A

Mixture

77
Q

Components can be separated by chemical means

A

Compounds

78
Q

Components do not lose identity.

A

Mixture

79
Q

Constituents can be separated by chemical means

A

Compounds

80
Q

Components may be separated by mechanical means.

A

Mixtures

81
Q

Composed of two or more substances that are chemically combined.

A

Compound

82
Q

Composed of two or more substances that are not chemically combined.

A

Mixture

83
Q

It is a chemical compound always contains exactly the same proportion of elements by mass.

A

Law of Definite Proportions

84
Q

It is a law when two elements combine to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers

A

Law of Multiple Proportions

85
Q

Elements combine in the ratio of
their combining weights or chemical equivalents; or in some simple multiple or sub-multiple of that ratio.

A

Law of Combining Weights

86
Q

Law of Combining Weights is also called

A

Also called the Law of Reciprocal Proportions or Law of Equivalents

GEN CHEM (2 decks)

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