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NMAT 2021 > Chemistry 1 > Flashcards

Chemistry 1 Flashcards

1
Q

anything that has mass and occupies space

A

Matter

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2
Q

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

A

Mixtures

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3
Q

change of state or phase

A

Physical Change

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4
Q

transformation in which substances are converted into other substances

A

chemical change

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5
Q

a substance composed of two or more elements chemically compounded into other substances

A

compound

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6
Q

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

A

element

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7
Q

the total mass of the products of a chemical reaction is the same as the total mass of the reactants

A

law of conservation of mass

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8
Q

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

A

law of definite composition (law of definite proportions)

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9
Q

when two elements from 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

A

law of multiple proportions

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10
Q

the number of protons in the nucleus

A

Atomic Mass

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11
Q

number of protons + number of neutrons

A

mass number

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12
Q

atoms of the same element with different mass numbers

A

Isotopes

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13
Q

exactly 1/12 the mass of carbon-12 atom

A

atomic mass unit (amu)

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14
Q

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

A

Atomic mass (weight)

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15
Q

quantity of a given substance that contains as many molecules or formula units as the number of atoms in exactly 12 g of carbon-12: consists of 6.02x10^23 particles

A

Mole (mol)

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16
Q

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

A

Molar mass

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17
Q

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

A

Mass% of A

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18
Q

definite group of atoms that are chemically bonded together

A

Molecule

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19
Q

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

A

Ion

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20
Q

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

A

Chemical Formula

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21
Q

formula with the smallest integer

A

empirical formula

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22
Q

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

A

Molecular Formula

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23
Q

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

A

Stoichiometry

24
Q

reactant that is entirely consumed when a reaction completes

A

Limiting Reactant or Limiting Reagent

25
Q

quantity of product that is calculated from when all of the LR reacts

A

Theoretical Yield

26
Q

amount of product actually obtained in a reaction

A

Actual Yield

27
Q

model that describes that the protons and neutrons are in the nucleus while the electrons are outside the nucleus

A

Nuclear Atomic Model

28
Q

the 4 quantum numbers

A

n (principal quantum number), l (azimuthal quantum number), mL (magnetic quantum number), mS (spin quantum number)

29
Q

identifies the shell or level to which the electron belongs to n = 1, 2, 3, 4….

A

Principal Quantum Number

30
Q

identifies the subshell s=0 p=1 d=2 f=3

A

Azimuthal Quantum Number

31
Q

gives the shape of the subshell; +1, 0, -1

A

Magnetic Quantum Number

32
Q

orientation of atomic orbital spin quantum number; +1/2 or -1/2

A

Spin Quantum Number

33
Q

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

A

Heisenberg’s Uncertainty Principle

34
Q

principle that states that no two electrons in the same atom may have the same set of all 4 quantum numbers

A

Pauli’s Exclusion Principle

35
Q

rule which states that in the ground state of an atom, electrons are distributed among the orbitals of a subshell in a way that gives the maximum number of unpaired electrons with parallel spins

A

Hund’s Rules of Multiplicity

36
Q

principle which states that a scheme used to reproduce the electronic configurations of atoms by successively filling subshell with electrons in a specific order (orbitals with lower energy first)

A

Aufbau Principle

37
Q

type of chemical bond formed by the transfer of electrons to form ions

A

Electrocovalent bond (ionic bond)

38
Q

type of chemical bond formed by the sharing of electrons between atoms

A

Covalent bond

39
Q

type of chemical bond characterized by equal sharing of a pair of electrons in diatomic molecules consisting of identical atoms in identical atoms with identical neighbors

A

Non-polar covalent bond

40
Q

type of chemical bond characterized by unequal sharing of a pair of electrons in identical atoms with different neighbors when two bonded atoms are dissimilar

A

Polar covalent bond

41
Q

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

A

Metallic Bond

42
Q

gases consist of particles in constant motion, gases are mostly empty space, particles exert pressure when colliding with container, particles don’t interact, molecular speed is proportional to temperature

A

Kinetic Molecular Theory

43
Q

the ideal gas law equation

A

PV=nRT

44
Q

pressure of vapor in equilibrium with a liquid at a given temperature

A

Vapor Pressure

45
Q

temperature at which the vapor pressure of a liquid is equal to the external pressure

A

Boiling Point

46
Q

resistance to the external pressure

A

Viscosity

47
Q

measure of the inward force on the surface of the liquid caused by the intermolecular forces of attraction

A

Surface tension

48
Q

atoms or molecules held together by intermolecular forces

A

Molecular solids

49
Q

positive cores of atoms held together by a sea of electrons

A

Metallic Solids

50
Q

cations and anions held together by the electrical attraction of opposite charges

A

Ionic Solids

51
Q

atoms held together in large networks or chains by covalent bonds

A

Covalent Network Solids

52
Q

a characteristic of a covalent bond which results when two atoms of different electronegatives form a covalent bond such that the electrons are not equally shared between them (with net dipole moment)

A

Polarity

53
Q

energy can be converted from one form into another, but it can neither be created nor destroyed

A

First law of thermodynamics

54
Q

every spontaneous change is accompanied by an increase in entropy

A

Second law of thermodynamics

55
Q

reactions tend to seek a minimum in energy and a maximum in randomness

A

Gibbs Free energy

56
Q

at absolute zero the entropy of a perfect crystalline substance may be taken as zero

A

Third law of thermodynamics

NMAT 2021 (8 decks)

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