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chem Flashcards

1
Q

made up of very small particles (atoms/molecules) that are
in constant motion and are held together by attractive forces.

A

Matter

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2
Q

low KE

A

solid

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3
Q

very high KE

A

gas

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4
Q

loosely packed together

A

liquid

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5
Q

high density

A

solid

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6
Q

Their kinetic energy is just enough for
them to vibrate and rotate in their fixed
positions

A

solid

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7
Q

A gaseous mixture of positive ions and
electrons

A

plasma

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8
Q

Heat energy is converted
to KE and the particles
vibrate and rotate faster
about their fixed
positions

A

melting

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9
Q

When the temperature is
low, the particles no
longer have enough energy
to move freely

A

freezing

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10
Q

occurs when
some particles of the
liquid have acquired
enough energy to break
away from their
attraction to the other
particles and escape as
gas.

A

evaporation

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11
Q

When gas is adequately
cooled, it changes into
a liquid.

A

condensation

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12
Q

When particles at the surface of a
solid acquire enough energy to
break away from the forces of
attraction in the solid, they escape
as gas.

A

sublimation

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13
Q

Occurs when the particles
of a gas condense
directly into a solid
without going through the
liquid state.

A

deposition

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14
Q

He proposed that if you kept cutting a
substance in half forever. Eventually you would end up with an
“uncuttable” particle.

A

Democritus

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15
Q

called the particles “atomos” meaning “indivisible” in
Greek

A

Democritus

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16
Q

revived
Democritus’s early ideas about the atom

A

John Dalton

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17
Q

“father of the modern atomic theory”

A

Dalton

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18
Q

discovered electrons

A

J.J Thomson

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19
Q

first subatomic particles to be identified

A

electrons

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20
Q

proposed the plum pudding model of the atom

A

Thomson

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21
Q

discovered nucleus

A

Ernest Rutherford

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22
Q

all the positive charge of an
atom is concentrated in a small central area.

A

nucleus

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23
Q

suggested that electrons travel around the
nucleus in definite paths

A

Niels Bohr

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24
Q

stated that electrons do not move in set
paths around the nucleus, but in waves

A

Erwin Schrodinger

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25
Q

clouds of probability

A

orbitals

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26
Q

The lightest of all three subatomic
particles. In fact, it is so light that it
has no great effect on the mass of
the atom

A

electron

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27
Q

It carries a net charge of negative
one (-1)

A

electron

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28
Q

Carries one positive electric
charge (+1)

A

proton

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29
Q

what subatomic particle was the first to observe by Eugene
Goldstein

A

proton

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30
Q

Has no net electrical charge

A

neutron

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31
Q

how to get neutron?

A

subtract mass number to atomic number

32
Q

In the periodic table, high energy = ?

A

period

33
Q

In the periodic table, valence electron = ?

A

group

34
Q

region of space around the nucleus where the electron is most likely to be found

A

atomic orbitals

35
Q

refers to the assignment of all the electrons in an atom into specific shells (energy levels) and subshells (sublevels)

A

Electron Configuration

36
Q

known as “building-up” principle, states that electron’s occupy orbitals in order of increasing energy

A

Aufbau Principle

37
Q

only 2 electrons can occupy each orbital and there must have opposite spins

A

Pauli’s Exclusion Principle

38
Q

electrons will half-fill each of the available equivalent orbitals before filling the second half of each orbital

A

Hund’s Rule

39
Q

(True or False) Does the energy increases as the distance of the orbit from the nucleus decreases?

A

false

40
Q

The orbits also known as shells or ?

A

energy levels

41
Q

If electron received extra energy, it can jump into a higher energy level, this is also called ?

A

excited state

42
Q

The electron in the excited state can return to its original lower energy level or _____ by releasing discreet amount of energy in the form of light

A

ground state

43
Q

The probability of finding the electrons is greatest at a certain specified distances from the nucleus called?

A

energy levels (electron shells)

44
Q

a quantitative measurement of the
energy change when an electron is added to a neutral gaseous
atom.

A

electron affinity

45
Q

(true or false) A more negative electron affinity value indicates higher
affinity?

A

true

46
Q

(true or false) The trend of the electron
affinity increases from left to
right and bottom to top throughout the periodic
table?

A

true

47
Q

Why is the trend of the electron
affinity increases from left to
right throughout the periodic
table?

A

due to a nuclear change
because of the attraction of the
electrons to the nucleus

48
Q

Why is the trend of the electron
affinity increases from bottom to
top throughout the periodic
table?

A

due to the atomic
size.

49
Q

used to find out if an atom or molecule will
be an electron acceptor or an electron donor and if a pair of
reactants will participate in charge transfer reaction

A

electron affinity

50
Q

the ability of an atom to lose electrons and become positive ions.

A

metallic character

51
Q

the tendency of an element to easily accept electrons and form
negative ions or anions.

A

nonmetallic character

52
Q

known as donors, (donates electrons and from positive ions)

A

metallic character

53
Q

known as acceptors, (accepts electrons and forms negative ions)

A

nonmetallic character

54
Q

true or false. When ionization energy increases, it requires more energy to lose valence
electrons.

A

true

55
Q

true or false. Non metals have high ionization energy and metals have low
ionization energy.

A

true

56
Q

directly proportional to non
metallic character and
indirectly proportional to
metallic character

A

ionization energy/electronegativity

57
Q

Tendency of an atom or a functional group to attract electrons toward itself

A

electronegativity

58
Q

true or false. As the atomic radius increases, so does a metal’s ability to lose electorns because of
distance.
This makes them directly proportional. While it is indirectly proportional to non metallic
character

A

true

59
Q

In the periodic table, trend of metallic character?

A

increases from top right to bottom left

60
Q

In the periodic table, trend of nonmetallic character?

A

increases from bottom left to top right

61
Q

a process that
involves the removal of electrons
present in an orbit outside the
atom.

A

Ionization

62
Q

the minimum energy required to
remove a loosely bound electron of an atom in the
gaseous state. It measures the capability of an atom to
lose an electron during a chemical reaction. It is opposite
to electron affinity

A

Ionization energy

63
Q

It would take energy for the positively charged nucleus
to attract the negatively charged electrons and to
completely remove an electron from the outermost shell
from a neutral atom

A

Ionization energy

64
Q

Since energy is added to the system, the process is
endothermic, and the ionization values are positive. True or false?

A

True

65
Q

Is Ionization energy is ALWAYS POSITIVE?

A

True

66
Q

Since only one electron is removed, the
ionization energy is also known as the _______

A

first ionization energy

67
Q

The farther away an electron is from
the nucleus, the easier it is to pull it
away. TRUE OR FALSE

A

true

68
Q

The larger the effective nuclear charge,
the less energy it takes to release an
electron

A

false

69
Q

Ionization energy, electronegativity and electron affinity has same trend in periodic table?

A

Yes

70
Q

Non metals have high electronegativity, making it easier to attract electrons. TRUE OR FALSE

A

true

71
Q

a measure of how strongly an atom attracts
the shared electrons in a chemical bond.

A

Electronegativity

72
Q

The concept of electronegativity was first introduced by Linus
Pauling and is commonly measured using ______ with values ranging from approximately 0.7 to 4.0.

A

Pauling scale

73
Q

How electronegativity works?

A

The greater the electronegativity of an atom the
stronger its ability to attract shared electron.

74
Q

Why are noble gases not included in electronegativity?

A

Noble gases (Group 18) are not included in discussions of electronegativity trends because they typically do not form chemical bonds due to their stable electronic configurations. As such, they have no tendency to attract additional electrons and thus have extremely low electronegativity values.

75
Q

The most electronegative element is ________, with a Pauling electronegativity value of 3.98,
while the least electronegative elements are typically found among the alkali metals, such as
_______, with a value of approximately 0.7.

A

Flourine, Cesium

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