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GEN CHEM > ATOMS, MOLECULES AND IONS > Flashcards

ATOMS, MOLECULES AND IONS Flashcards

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1
Q

Greek philosopher who had the idea that al matter consisted of minute particles

A

Democritus

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2
Q

he coined the term atomos

A

Democritus

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3
Q

The scientist who provided precise and detailed description of the building block of matter

A

John Dalton

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4
Q

John Dalton’s atomic theory:

A
  1. An element is made up of extremely small, indestructible particles called atom
  2. Atoms of the same element have the same chemical properties
  3. Compounds are made up of atoms of more than one type of element
  4. Atoms are rearranged to produce different substances
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5
Q

3 fundamental laws of matter

A
  1. law of conservation of mass
  2. law of constant composition or definite proportions
  3. law of multiple proportions
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6
Q

explains that elements combine in ratios of simple whole numbers to form a compound

A

law of constant composition or definite properties

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7
Q

explains that 2 or more elements react to form two or more different compounds, with one fixed or constant element

A

law of multiple proportions

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8
Q

he carefully measured both the reactants and the products of chemical reactions

A

Antoine-Laurent Lavoisier

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9
Q

states that matter is neither created nor destroyed in a chemical reaction

A

law of conservation of mass

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10
Q

this law states that in any chemical reaction, atoms are always conserved

A

law of conservation of mass

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11
Q

negatively charged subatomic particle

A

electron

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12
Q

discovered electrons

A

J.J. Thomson

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13
Q

mass of electrons

A

9.11 x 10^-28g

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14
Q

positive charged subatomic particle

A

Proton

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15
Q

he’s famous for using the Gold foil experiment

A

Ernest Rutherford

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16
Q

mass of proton

A

1.6726 x 10^-24g

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17
Q

protons is located at the center of atom

A

nucleus

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18
Q

discovered protons

A

Ernest Rutherford

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19
Q

electrically neutral subatomic particle

A

neutron

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20
Q

discovered neutrons

A

James Chadwick

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21
Q

mass of neutrons

A

1.6749 x 10^-24g

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22
Q

contains a nucleus composed of protons and neutrons and electrons moving around the nucleus

A

atoms

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23
Q

2 ways to describe an atom quantitatively based on the number of specific subatomic particles:

A
  1. atomic number
  2. atomic mass
24
Q

equal to the number of protons in an atom

A

atomic number

25
Q

total amount of particles

A

mass number

26
Q

atoms with the same number of protons but different number of neutrons

A

isotopes

27
Q

isotopes that do not undergo radioactivity and do not disintergrate

A

Stable isotopes

28
Q

those that exhibit radioactivity

A

unstable isotopes

29
Q

has the same number of electrons and protons

A

nuetral atom

30
Q

neutrality is lost during chemical changes in which an atom either lose or gain an electron to give an electrically charged species called

A

ions

31
Q

is lost during chemical changes in which an atom either lose or gain an electron to give to ions

A

neutrality

32
Q

when an atom gains an electron, it becomes negatively charged and is then called

A

anion

33
Q

when an atom gives off an electron its charge becomes positive and is then called

A

cation

34
Q

a collection of 2 or more atoms held in a specific arrangement due to sharing of electrons and acts as a single unit is called

A

molecule

35
Q

combination of molecules of the same element

A

diatomic molecule

36
Q

aggregate of 2 or more types of atoms

A

diatomic

37
Q

shows the type of atom and the number constituting a certain molecule

A

Molecular formula

38
Q

shows the order in which the atoms in the molecule are bonded

A

structural formula

39
Q

type of perspective drawing that shows the 3 dimensional orientation of molecules

A

Ball and Stick Model

40
Q

similar to ball and stick model but the line denotes the sharing of electrons is omitted

A

Space-filling model

41
Q

represents 3 dimensions and is used primarily to distinguish among optical isomers

A

Perspective formula

42
Q

formula where the symbols of atoms are listed in order as they appear in the molecule’s structure

A

Condensed formula

43
Q

uses solid or dashed wedged bonds to depict the orientation of atoms in a molecule

A

Natta projection

44
Q

represents bonds using solid lines

A

Skeletal formula

45
Q

called electron dot structure; dots represent bonding of electrons and unpaired electrons

A

Lewis structure

46
Q

used to illustrate structures or linear monosaccharides

A

Fischer projection

47
Q

chair-like conformation commonly used to view structures of sugars

A

Cyclohexane conformation

48
Q

used to represent structures of cyclic sugars

A

Haworth projection

49
Q

used to illustrate a single bond between 2 carbon atoms

A

Newman and Sawhorse projections

50
Q

The ___________ of a compound denotes the exact number of atoms present in a molecule

A

molecular formula

51
Q

does not provide the exact number of atoms composing the molecule

A

empirical formula

52
Q

are compounds made up of cation and anion

A

ionic compound

53
Q

formed when cation and an anion combine due to the transfer of electrons

A

ionic bond

54
Q

formed when 2 or more nonmetals bond by sharing valence electrons

A

covalent compound

55
Q

a class of acid composed of hydrogen and a nonmetal

A

binary acid

56
Q

made up of hydrogen, oxygen and a nonmetal

A

ternary acid

57
Q

ternary acid also refers to

A

oxoacid

GEN CHEM (7 decks)

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