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Chemistry for Engineers > Module 1 > Flashcards

Module 1 Flashcards

1
Q

refers to the structure of an atom comprising a nucleus

A

atomic structure

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2
Q

what is the center of the atom

A

nucleus

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3
Q

what atom is a positively charged

A

protons

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4
Q

an atom that is neutral charged

A

neutrons

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5
Q

the negatively charged particles

A

electrons

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6
Q

smallest atomic arrangement is

A

unit cell

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7
Q

plays an important role in determining the microstructure and behavior of a solid

A

atomic arrangement

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8
Q

are structures that range between 1 nm and 100 nm in at least one dimension

A

nanostructure

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9
Q

material structures seen at the micro level

A

microstructure

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10
Q

they are structures of an object, organism, or material as revealed by a microscope

A

microstructure

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11
Q

the structure of a material at a macroscopic level where the length scale is >100 um

A

macrostructure

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12
Q

what are the features that constitute macrostructure

A

PSIE
Porosity, Surface coatings, Internal microcracks, and external microcracks

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13
Q

composed of a nucleus surrounded by electrons

A

atom

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14
Q

it contains neutrons and positively charged protons and carries a net positive charge

A

nucleus

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15
Q

nucleus contains neutrons and positively charged protons and carries what charge?

A

a net positive charge

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16
Q

the negatively charged electrons are held to the nucleus by an?

A

electrostatic attraction

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17
Q

the charge of number of an atomic nucleus which is equal to the number of protons in each atom

A

Atomic number

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18
Q

equal to the total mass of the average number of protons and neutrons in atomic mass units, also the mass of the grams of the Avogadro’s constant

A

atomic mass

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19
Q

value of Avogadro’s constant

A

6.022 x 10^23 mol

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20
Q

formula in calculating the number of atoms

A

Number of atoms= (avogadro’s constant/ atomic mass of an element)

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21
Q

the energy level to which each electron belongs is identified by for quantum numbers

A
  1. principal quantum number (n)
  2. the azimuthal or secondary quantum number (l)
  3. the magnetic quantum number (m)
  4. the spin quantum number (ms)
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22
Q

is assigned integer values 1,2,3,4,5.. that refer to the quantum shell to which the electron belongs

A

principal quantum number (n)

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23
Q

a set of fixed energy levels to which electrons belong

A

quantum shell

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24
Q

a quantum number for an atomic orbital that determines its orbital angular momentum and describes the shape of the orbital

A

azimuthal quantum number (l)

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25
it determines the number of energy levels in each quantum shell
azimuthal quantum number (l)
26
specifies the orientation in space of an orbital of a given energy (n) and shape (l). this number divides the subshell into individual orbitals which hold the electrons
magnetic quantum number (mi)
27
describes the intrinsic spin of an electron.
spin quantum number (ms)
28
for electron it has two possible values
ms= -1/2 and +1/2
29
states that two or more identical particles with half- integer spins cannot occupy the same quantum state within a quantum system simultaneously
pauli exclusion principle
30
a graphical device that predicts deviations from the expected ordering of the energy levels
Aufbau principle
31
electrons will occupy each orbital of a given energy level singly before the orbitals are doubly occupied
Hund's rule
32
an electron in the outer shell associated with an atom
valence electron
33
describes the tendency for an atom to attract shared electrons when forming a chemical bond
electronegativity
34
the typical distance from the center of the nucleus to the outermost electron
atomic radius
35
the minimum energy required to remove the most loosely bound electron of an isolated gaseous atom
ionization energy
36
the ability of an atom to accept an electron and the energy change that results from adding an electron to a gaseous atom
electron affinity
37
Atomic radius_____ from left to right within a period. this is caused by the ____ in the number of protons and electrons across a period
decreases, increase
38
atomic radius______from top to bottom within a group. caused by electron shielding or principal quantum number, n.
increases
39
from ____to____ across a period of elements, electronegativity increases
left to right
40
from ___to___ down a group, electronegativity decreases
top to bottom
41
has the highest ionization energy of all elements
Helium
42
a metal that contains additions of one or more metals or non-metals
alloy
43
have good electrical and thermal conductivity
metals
44
have relatively high strength, high stiffness, ductility, and shock resistance
metals and alloys
45
can be defined as inorganic crystalline materials typically based on combinations of many elements.
ceramics
46
are plastics that are primarily based on carbon. have a very good strength-weight ratio, not suitable for use at high temperatures
polymers
47
are good electrical and thermal insulators
polymers
48
has electrical conductivity between that of ceramic insulators and metallic conductors
semiconductors
49
four types of chemical bonds
metallic bonds, covalent bonds, ionic bonds, van der waals bonds
50
a type of chemical bond formed between positively that donate their valence electrons to form a sea of electrons surrounding the atoms
metallic bond
51
refers to the ability of materials to be stretched or bent permanently without breaking
ductility
52
difference in electronegativity of ionic bond
>2.0
53
difference in electronegativity of covalent bond
<1.7
54
difference in electronegativity of polar covalent bond
>0.5
55
difference in electronegativity of non-polar covalent bond
<0.5
56
in this bond, one atom gives up its electron to the other atom and forms two ions with opposite charge
ionic bond
57
two atoms share two electrons if there difference in electronegativity is <1.7
covalent bond
58
difference in electronegativity >0.5
polar covalent bond
59
difference in electronegativity <0.5
non-polar covalent bond
60
a relatively weak attractive forces that act on neutral atoms and molecules and that arise because of the electric polarization
Van der Waals Force
61
types of van der waals interactions:
LDK London forces, Debye interaction, and Keesom forces
62
if the interaction are between two dipoles that are induced in atoms or molecules
london forces
63
when an induced dipole interacts with a molecule that has a permanent dipole moment
debye interaction
64
if the interaction are between molecules that permanently polarized
Keesom force
65
the equilibrium distance between atoms is cause by a balance between repulsive and attractive forces
interatomic spacing
66
the energy required to create or break the bond
binding energy
67
the unit measurement of an objects or substance resistance to being deformed elastically when a stress is applied to it
modulus of elasticity
68
refers to the rate at which a material expands with increase in temperature
coefficient of thermal expansion
69
the maximum stress that can be applied before a material begins to change shape permanently
yield strength
70
the maximum stress that a material can withstand while being stretched or pulled before breaking
tensile strength
71

Chemistry for Engineers (4 decks)

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