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GEN CHEM > NMAT > Flashcards

NMAT Flashcards

1
Q

Matter

A

anything that has mass and occupies space

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2
Q

Mixtures

A

combinations of 2 or more substances in which each substance retains its own chemical identity and properties

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3
Q

Compound

A

substance composed of 2 or more elements chemically combined in fixed proportions

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4
Q

Element

A

substance that cannot be decomposed by any chemical reaction into simpler substances

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5
Q

Law of Conservation of Mass

A

total mass of the products of a chemical reaction is the same as the total mass of the reactants (mass remains constant during chemical reaction)

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6
Q

Law of Conservation of Mass

A

total mass of the products of a chemical reaction is the same as the total mass of the reactants (mass remains constant during chemical reaction)

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7
Q

Law of Definite Composition

A

the elemental composition of a pure compound is always the same, regardless of its source

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8
Q

Law of Multiple Proportions

A

2 elements form more than one compound, the masses of one element in these compounds for a fixed mass of the other element are in ratios of small whole numbers

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9
Q

Atomic Number

A

no. of protons in nucleus

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10
Q

Mass number

A

protons + neutrons

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11
Q

Isotopes

A

atoms of the same element with different mass numbers

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12
Q

Atomic Mass Unit

A

exactly 1/12th the mass of a carbon-12 atom

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13
Q

Atomic Mass

A

average mass of the atoms of an element in amu; mass in g of one mol of the element

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14
Q

Mole

A

quantity of a given substance that contains as many molecules or formula units as the no. of atoms in exactly 12 g of carbon-12; consists of 6.02 x 10^23 particles

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15
Q

Molar Mass

A

mass of one mol of substance; in g it is numerically equal to the formula mass (weight) in atomic mass units

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16
Q

Mass % of A

A

(mass of A in whole/mass of the whole) x 100%

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17
Q

Molecule

A

definite group of atoms chemically bonded together

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18
Q

Ion

A

electrically charged particle obtained from an atom or chemically bonded group of atoms by adding or removing electrons

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19
Q

Chemical formula

A

notation that uses atomic symbols with numerical subscripts to convey the relative proportions of atoms of the different elements in the substance

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20
Q

Empirical Formula

A

formula with the smallest integer subscripts

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21
Q

Molecular Formula

A

chemical formula that gives the exact number of different atoms of an element in a molecule

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22
Q

Molecular Mass/Weight

A

the sum of the atomic masses/weights of all the atoms in a molecule

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23
Q

Formula Mass/Weight

A

the sum of the atomic masses/weights of all atoms in a formula unit of the compound, molecular or not

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24
Q

Empirical Formula Mass/Weight

A

the sum of the atomic masses divided by the weights of all the atoms in an empirical formula

25
Q

Molecular Formula

A

n x Empirical Formula
where n = molecular or formula weight / empirical formula weight

26
Q

Stoichiometry

A

calculation of the quantities of reactants and products involved in a chemical reaction

27
Q

Limiting Reactant or Reagent

A

reactant that is entirely consumed when a reaction is completed

28
Q

Theoretical Yield

A

quantity of product that is calculated to form when all of the LR reacts

29
Q

Actual Yield

A

amount of product actually obtained in a reaction

30
Q

Percentage Yield

A

(actual yield / theoretical yield) x 100%

31
Q

________ Atomic Theory

A

Dalton’s

32
Q

Main postulates of the atomic theory

A

Matter is composed of very tiny or microscopic particles called atom

  1. Atom is an indivisible particle
  2. Atom can neither be created nor destroyed
  3. Atoms of an element are identical in size, shape, mass, and in other properties
  4. Atoms of different elements are different in their properties
  5. Atoms combine with each other in small whole numbers
  6. All chemical reactions are due to the combination or separation of atoms
33
Q

Defects in Dalton’s Theory

A
  • Atoms can be divided into a number of sub-atomic particles (electrons, protons and neutrons)
  • Atoms of an element may be different in their masses
  • Not all compounds have small number of atoms
  • Atoms can be destroyed by fission process (atom bomb, nuclear reactor)
34
Q

Nuclear Atomic Model

A

Protons and Neutrons in the nucleus; electrons outside the nucleus

35
Q

Heisenberg’s Uncertainty Principle

A

it is impossible to determine simultaneously the exact position and the exact momentum of a fast moving body like an electron

36
Q

Pauli’s Exclusion Principle

A

no 2 electrons in the same atom may have the same set of all 4 quantum numbers

37
Q

Hund’s Rule of Multiplicity

A

in the ground state of an atom, electrons are distributed among the orbitals of a sub-shell in a way that gives the maximum number of unpaired electrons with parallel spins

38
Q

Aufbau Principle (Building up Principle)

A

a scheme used to reproduce the electronic configurations of atoms by successively filling sub-shells with electrons in a specific order (orbitals with lower energy first)

39
Q

Atomic Size

A

within a period - decreases from left to right
within a group - increases from top to bottom

40
Q

Size of Cation

A

within a period - decreases from left to right
within a group - increases from top to bottom

41
Q

Size of Anion

A

within a period - decreases from left to right
within a group - increases from top to bottom

42
Q

Ionization Energy

A

energy needed to remove an electron from a gaseous atom in the ground state

within a period - increases from left to right
within a group - decreases from top to bottom

43
Q

Electron Affinity

A

energy change when an electron is added to a gaseous atom in the ground state

within a period - increases negative value from left to right
within a group no clear trend

44
Q

Basicity of Metal Oxides

A

within a period - decreases from left to right
within a group - increases from top to bottom

45
Q

Acidity of Non-metal Oxides

A

within a period - increases from left to right
within a group - decreases from top to bottom

46
Q

Metallic (Reducing) Property

A

within a period - decreases from left to right
within a group - increases from top to bottom

47
Q

Non-Metallic (Oxidizing) Property

A

within a period - increases from left to right
within a group - decreases from top to bottom

48
Q

Electronegativity

A

measure of the ability of an atom in a molecule to draw bonding electrons to itself

within a period - increases from left to right
within a group - decreases from top to bottom

49
Q

Electrovalent Bond (Ionic)

A

formed by transfer of electrons to form ions

50
Q

Covalent Bond

A

formed by sharing of electrons between atoms

51
Q

Formal Charge and what does it mean?

A

Group number - number of unshared electrons - number of covalent bonds

the higher the bond order, the shorter the bond length and the greater the bond strength

52
Q

Metallic Bond

A

a crystal of the metal consists of a regular arrangement of the positive ions, and the valence electrons move throughout the crystal attracted to the positive cores of all the positive ions

53
Q

Non-polar Covalent Bond

A

equal sharing of a pair of electrons in diatomic molecules consisting of identical atoms in identical atoms with identical neighbors

54
Q

Polar Covalent Bond

A

unequal sharing of a pair of electrons in identical atoms with different neighbors when two bonded atoms are dissimilar

55
Q

What kind of molecule has symmetrical polar bonds?

A

non-polar molecules

56
Q

What kind of molecule has asymmetrical polar bonds?

A

Polar molecules

57
Q

Shape of molecule with 6-2 Bonding e-pairs

A

6: octahedral
5: square pyramidal
4: square planar
3: T-shaped
2: linear

58
Q

Hybrid Orbitals

A

mixing of atomic orbitals to form a hybrid; the number of hybrid orbitals is equal to the number of pure atomic orbitals that mixed

59
Q

Phases of Matter

A
  1. Ion-dipole
  2. Dipole-dipole
  3. London forces / Van der Waals forces
  4. H-bonding

GEN CHEM (1 decks)

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