Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Materials > Atomic structure and interatomic bonding Chpt 2 > Flashcards

Atomic structure and interatomic bonding Chpt 2 Flashcards

1
Q

What is the net force

A

sum of attractive and repulsive forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What do the attractive force depend on

A

depends on type if bonding that exists

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What causes repulsive forces?

A

when negatively charged electron clouds interact with small distances and when outer electron shells overlap

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When does further pushing or pulling from atoms prevented by attractive and repulsive forces

A

.3nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are the primary and secondary bonding forces

A

ionic, covalent and metallic

van der waals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What subatomic particle has a smaller massq

A

electorn

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Where is the atomic number located?
atomic mass?

A

bottom left
top left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Explain carbon-15

A

number of carbon is 12 but has 3 neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Unit for atmoic mass. how is it defined

A

amu

1/12 of atomic mass of most common isotope carbon atom (6protons 6 neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Whatis the z number?

A

protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Whats bhors atomic model

A

think rings n=3 etc

electrons in orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the wave-mechanical model?QAs`

A

tells us that electrons move in fuzzy orbits, not circular

Can only tell you probability of finding them at various locations around the nucleus

electrons considered to have wave and particle like characteristics

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the Quantum-mechanical principle

A

Energies of electrons are quantized

principles that govern sys of atomic and subatomic entities

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are subatomic particle charges measured in

A

Coulombs

attractive bonding forces are coulombic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Charge of pr and el

A

1.602 x 10^-19C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What letter is the atomic number

A

Z

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Atomic mass vs atomic mass unit vs atomic weight

A

atomic mass: neutrons v protons

1/12 of atomic mass of most common carbon isotope carbon-12

average weight of the atom’s isotopes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What letter is atomic mass

A

A

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

mole is?

A

6.022 x 10^23

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

1amu/atom(or molecule) = 1g/mole

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Can electrons have different energies?

A

YES! they can change energy orbitals and have different energies in different moments

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Pauli exclusion principle

A

No two electons in same atom have identical values for all four of their quantum numbers

18
Q

electron configuration

A
19
Q

Describe all four quantum numbers

A

Principle Quantum Number (n): tells you the energy level of an electron inside an atom (size of electron orbital)

Angular Momentum Quantum Number (l): describes the shape of the sublevel within an energy level
s (shere) - 0 has one orbital
p (3D infinity) - 1 has 3 orbitals
d (4 flat bubbles) - 2 has 5 orbitals
f (two bubles as axis) - 3 has 7 orbitals

Magnetic Quantum Number (m_l): describes orbital within sublevel
-l <= m_l <= l

Electron Spin (m_s): can be +1/2 or -1/2
an electron in an orbital can either go up or
down
ex: 3d^8 is a -1/2 or +1/2 depending on if
you start with all down or up arrows

https://www.youtube.com/watch?v=eRIN9CPDrpo

20
Q

Whats ground state

A

the lowest energy an atom can be in

21
Q

Are noble gases reactive or unreactive

A

unreactive

22
Q

name the column names

A

8th: noble (inert) gases
7th: halogens
4-6: other nonmetals (including hydrogen)
3rd: metalliods ( horizontal pattern)
between 2 and 3: transition metals
2nd: alkaline earth metals
1st: alkali metals
study periodic table
upper low: lanthanides
lower low: actinides

23
Q

describe the periodic table trend with spdf

A
24
Q

Electropositive vs electronegative and periodic trend

A

+: willing to give up electron
-: readily accept electrons

more electronegative as you move to the right of P.T.

25
Q

Ionic vs covalent bonding

A

metal and nonmetal bonding (transferring electrons requires large electronegative difference nondirectional bond. dissolve in water easily and other polar solvents. Tend to form crystalline solids with high melting temperature

between atoms of small electronegative differences (near in periodic table). orbital overlap. Highly directional bonding bc they bond in the direction of greatest orbital overlap (diamonds, polymeric molecules like ethylene, ceramics and semi-conductors)

26
Q

Where do electrons go when they have more energy?

A

higher orbital

27
Q

What does the group number tell you about an atom

A

the number of electrons available

28
Q

when atoms are at r0?

A

atom is in equillibrium

29
Q

Whats bonding energy E_o?

A

amount of energy required to break a mole of molecules into component atoms

30
Q

Equilibrium is reached in forces when bonding energy is minimized

A
31
Q

cation vs anion

A

cation (+)
anion (-)

32
Q

What are nondirectional bonds

A

when the direction of the attraction between atoms do not matter.

33
Q

Why do electrons transrer in ionic bonding?

A

atoms want to be at a ground state level, meaning they want to reduce the energy of the system.

34
Q

how do you name an ionic compound

A

name the metal first, then the nonmetal second

35
Q

What is mtallic Bonding?

A

valence electrons detached from atoms and swim in electron sea that glues ions together.

Non-directional bonding

metal is held together by strong force of attraction between positive nuclei and delocalized electrons

36
Q

What is non-directional bonding

A

probability of sharing electron is equal in all directions

37
Q

What happens to nuclei when valence elctron are in elecytorn sea?

A

nucleus and core electrons for ion cores with net positive charge,

38
Q

what are delocalized electrons

A

valence electrons that don’t belong to any one atom.

39
Q

What is the van de Waals

A

weak attractive force between dipoles

like when sodium chloride positive side attracts negative other atom

secondary attractive

40
Q

what are dipoles

A

pair of electric charges or magnetic poles of equal but opposite charge, separated by small distance

41
Q

Whats permanent dipole?

A

like when sodium chloride positive side attracts negative other atom

all due to asymmetrical arrangment of positive and negative regions

strongest secondary bond

42
Q

How do polar molecules affect nonpolar molecules?

A

makes them polar, lol

bond is formed due to attraction between permanent and induced dipoles

43
Q

can electrically symmetric molecules and atoms create a dipole

A

yes. fluctiations in electron density (fluctuating dipoles)

weakest bond

44
Q

what bonding in each material?

metals
ceramics
polymers
semiconductors

A

metallic
ionic/covalent
covalent and secondary
covalent or covalent/ionic

45
Q

periodic trend for atomic size, electronegativity, ionization

A
46
Q

calculate the ionic percentage of materials

A

IC% = {1-exp(-(0.25)(X_A-X_B)^2)}*100

X_A and X_B are the electronegativity of the elements in the materials

47
Q

table for bonding energies and melting temperatures

A
48
Q

look at last slide of week 3

A

Materials (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions