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Chemistry for Engineers > Module 1 > Flashcards

Module 1 Flashcards

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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
Q

it determines the number of energy levels in each quantum shell

A

azimuthal quantum number (l)

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26
Q

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

A

magnetic quantum number (mi)

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27
Q

describes the intrinsic spin of an electron.

A

spin quantum number (ms)

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28
Q

for electron it has two possible values

A

ms= -1/2 and +1/2

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29
Q

states that two or more identical particles with half- integer spins cannot occupy the same quantum state within a quantum system simultaneously

A

pauli exclusion principle

30
Q

a graphical device that predicts deviations from the expected ordering of the energy levels

A

Aufbau principle

31
Q

electrons will occupy each orbital of a given energy level singly before the orbitals are doubly occupied

A

Hund’s rule

32
Q

an electron in the outer shell associated with an atom

A

valence electron

33
Q

describes the tendency for an atom to attract shared electrons when forming a chemical bond

A

electronegativity

34
Q

the typical distance from the center of the nucleus to the outermost electron

A

atomic radius

35
Q

the minimum energy required to remove the most loosely bound electron of an isolated gaseous atom

A

ionization energy

36
Q

the ability of an atom to accept an electron and the energy change that results from adding an electron to a gaseous atom

A

electron affinity

37
Q

Atomic radius_____ from left to right within a period. this is caused by the ____ in the number of protons and electrons across a period

A

decreases, increase

38
Q

atomic radius______from top to bottom within a group. caused by electron shielding or principal quantum number, n.

A

increases

39
Q

from ____to____ across a period of elements, electronegativity increases

A

left to right

40
Q

from ___to___ down a group, electronegativity decreases

A

top to bottom

41
Q

has the highest ionization energy of all elements

A

Helium

42
Q

a metal that contains additions of one or more metals or non-metals

A

alloy

43
Q

have good electrical and thermal conductivity

A

metals

44
Q

have relatively high strength, high stiffness, ductility, and shock resistance

A

metals and alloys

45
Q

can be defined as inorganic crystalline materials typically based on combinations of many elements.

A

ceramics

46
Q

are plastics that are primarily based on carbon. have a very good strength-weight ratio, not suitable for use at high temperatures

A

polymers

47
Q

are good electrical and thermal insulators

A

polymers

48
Q

has electrical conductivity between that of ceramic insulators and metallic conductors

A

semiconductors

49
Q

four types of chemical bonds

A

metallic bonds, covalent bonds, ionic bonds, van der waals bonds

50
Q

a type of chemical bond formed between positively that donate their valence electrons to form a sea of electrons surrounding the atoms

A

metallic bond

51
Q

refers to the ability of materials to be stretched or bent permanently without breaking

A

ductility

52
Q

difference in electronegativity of ionic bond

A

> 2.0

53
Q

difference in electronegativity of covalent bond

A

<1.7

54
Q

difference in electronegativity of polar covalent bond

A

> 0.5

55
Q

difference in electronegativity of non-polar covalent bond

A

<0.5

56
Q

in this bond, one atom gives up its electron to the other atom and forms two ions with opposite charge

A

ionic bond

57
Q

two atoms share two electrons if there difference in electronegativity is <1.7

A

covalent bond

58
Q

difference in electronegativity >0.5

A

polar covalent bond

59
Q

difference in electronegativity <0.5

A

non-polar covalent bond

60
Q

a relatively weak attractive forces that act on neutral atoms and molecules and that arise because of the electric polarization

A

Van der Waals Force

61
Q

types of van der waals interactions:

A

LDK
London forces, Debye interaction, and Keesom forces

62
Q

if the interaction are between two dipoles that are induced in atoms or molecules

A

london forces

63
Q

when an induced dipole interacts with a molecule that has a permanent dipole moment

A

debye interaction

64
Q

if the interaction are between molecules that permanently polarized

A

Keesom force

65
Q

the equilibrium distance between atoms is cause by a balance between repulsive and attractive forces

A

interatomic spacing

66
Q

the energy required to create or break the bond

A

binding energy

67
Q

the unit measurement of an objects or substance resistance to being deformed elastically when a stress is applied to it

A

modulus of elasticity

68
Q

refers to the rate at which a material expands with increase in temperature

A

coefficient of thermal expansion

69
Q

the maximum stress that can be applied before a material begins to change shape permanently

A

yield strength

70
Q

the maximum stress that a material can withstand while being stretched or pulled before breaking

A

tensile strength

71
Q
A

Chemistry for Engineers (4 decks)

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