chem Flashcards

1
Q

it tells
how many molecular weights of solute are dissolved in
each “Liter” of solution

A

) Molar (M)

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2
Q

In the clinical laboratory, “water” always refers to

A

distilled water

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3
Q

contains more than the maximum amount
of solute that can be dissolved at that temperature

A

Supersaturated Solution

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4
Q

how much solute is dissolved
in one hundred parts (usually 100 ml) of the solution

A

Percent solutions

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5
Q

s a homogeneous part of a system separated
from other parts by physical boundaries.

A

Phase

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6
Q

material containing two or more substances

A

Mixture

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7
Q

the molecules or ions are so small (less
than 1 nm) that they cannot be seen and will remain
dispersed in the liquid

A

a true solution

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8
Q

When water is the solvent we say it is an

A

aqueous solution

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9
Q

Particular kind of matter with fixed
composition ,may be present in different states or phases

A

Substance

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10
Q

the solvents has only a small quantity of solute
dissolved in it

A

Dilute solution

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11
Q

The dissolving substance

A

solvent

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12
Q

………………… gives a liquid fluidity and causes it to take……………… in which it is stored.

A

Particle mobility, the shape of the container

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13
Q

it tells how many
equivalent weights of solute are dissolved in a “Liter” of
solution.

A

Normal (N)

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14
Q

The solvent has a large quantity of solute
dissolved in it

A

Concentrated solution

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15
Q

discrete, tiny, fundamental particles

A

atoms

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16
Q

The substance being dissolved in the solvent

A

solute

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17
Q

is anything that has mass and occupies space.

A

matter

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18
Q

This tells how many molecular weights of solute per Kg of
solvent.

A

Molal ( m )

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19
Q

It is a homogenous mixture of two or more substances

A

Solution

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20
Q

contains the maximum amount of solute that will
dissolve at that temperature.

A

Saturated solution

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21
Q

The elements were first arranged in this way in 1869 by ……………………, a Russian scientist.

A

Dimitri
Mendeleev

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22
Q

each box there is the symbol for the element
and, above it, a number called the

A

atomic number.

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23
Q

The elements in the modern periodic table are arranged in
order of increasing …………………

A

atomic number.

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24
Q

atoms of an element must be capable of
having ………….numbers of
neutrons

A

varying

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25
Q

electrons enter orbitals of equal energy singly
with the same spin before they become paired

A

Hund’s rule

26
Q

Two atoms with the same atomic number but
different atomic weights will be

A

isotopes

27
Q

 It shows all the chemical elements and contains a great deal
of useful information about them

A

periodic table

28
Q

there are three kinds of hydrogen atoms

A

hydrogen deuterium tritium

29
Q

l. The arrows denote the
property of ………….

A

spin

30
Q

the ………….. forces will attempt to keep each electrons as close to the nucleus as possible.
 there is a ……………..force operating between the two like charged ( - ) electrons.

A

attractive, repulsive

31
Q

why atoms have more empty
spaces

A

Because of the spaces between electrons
and the nucleus

32
Q

 A number is given below the symbol of the element.

A

atomic weight (atomic mass)

33
Q

is the body of matter under consideration.

A

System

34
Q

Mendeleev arranged the elements in this way because of …………………..of various “families” of
elements.

A

similarities in the chemical properties

35
Q

Mendeleev and Meyer arranged the elements in order of increasing atomic number………….. from left to right and so that the elements that reacted similarly were in the same ………………,

A

horizontally, vertical columns

36
Q

Mendeleev predicted the existence of
undiscovered elements based on the observation of ………………….

A

periodicity

37
Q

the metals shown
in the center of the periodic table. the inner levels are not always
completely filled, they are

A

transition metals non representative B
Group elements.

38
Q

Elements of similar properties are repeated …………….

A

periodically

39
Q

Electrons in the outermost level

A

valence

40
Q

specific patterns that are present in the periodic
table illustrating different properties of elements.

A

Trends

41
Q

the amount of energy needed to remove one electron
from each of the atoms in a gaseous sample.

A

Ionization energy

42
Q

It is the radius of the atom (distance between the
center of nucleus and the outermost energy level electrons)

A

Atomic size

43
Q

Relation between
Ionization energy
and atomic size is………………..

A

inversely

44
Q

: It is the ability of an atom to attract bonding pair
of electrons.

A

Electronegativity

45
Q

teasures the difference in electronegativity between two
atoms bonded with covalent bond.

A

Dipole Moments

46
Q

substance changes in appearance
but remains the same substance (by applying or removing
heat)

A

Physical change:

47
Q

A change that produces a new substance

A

Chemical change

48
Q

s the force that holds elements together in
compounds.

A

Chemical bond:

49
Q

Other elements strive to achieve eight valence
electrons

A

rule of octet rule
eigh

50
Q

gaining electrons

A

reduction

51
Q

losing electrons

A

oxidation

52
Q

Energy and matter cannot be created or
destroyed, they can only be transformed
or changed from one form to another.

A

Law of conservation
of energy and matte

53
Q

Ionic compounds form through………………..

A

electron transfer

54
Q

Simple ions are also called ……………………….

A

monoatomic ions,

55
Q

Ionic compounds are so named

A

because they are
combinations of ions.

56
Q

a charged species made
from many atoms.

A

polyatomic ion

57
Q

hen two or more nonmetals combine to form a molecule, no
electron transfer takes place

A

COVALENT BOND

58
Q

Certain elements (e.g. H2, O2, N2 and halogens) exist as…………………………. rather than individual atoms by sharing
their electrons in order to achieve a noble-gas
configuration

A

diatomic molecules

59
Q

The valence electrons not involved in bonding

A

nonbonding electrons or unshared pairs

60
Q

The bond formed when two electrons occupy such a molecular orbital
is known as

A

Sigma bond

61
Q
A