Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 101 > Octet rule > Flashcards

Octet rule Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards Physics 101 flashcards Psychology 101 flashcards AP® Chemistry flashcards Biology 101 flashcards Organic Chemistry 101 flashcards Periodic Table flashcards Sociology 101 flashcards
1
Q

Octet rule

  • what does it form
  • where does it occur
  • what does it provide
  • the electron pair…
A
  • covalent bonds
  • between 2 non metals
  • each provides an electron to the sharing relationship
  • spends time with both nuclei so each feels like they have an octet
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

In the simplest covalent molecule, H2, the H atoms

A
  • increase attraction as they move closer
  • share electrons to form a covalent bond
  • the new compound is called a molecule
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The need for an octet is so great for what?

A

H, O and S and group 17 elements that they do not exist as free atoms

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

How is the number of covalent bonds determined

A

from the number of electrons needed to complete an octet

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

in a methane (CH4) molecule…

A
  • the central C atom shares 4 electrons to attain an octet

- each H atom shares 1 electron with the carbon atom to become stable like He

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

Average bond lengths

  • C-H
  • N-H
  • O-H
A
  • 109 pm
  • 101 pm
  • 96 pm
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What happens when sharing one pair does not make an octet?

  • in a single bond
  • in a double bond
  • in a triple bond
A
  • one pair of electrons is shared
  • 2 pairs of electrons are shared
  • 3 pairs of electrons are shared
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

In an oxygen molecule…

A
  • each O atom shares 2 electrons
  • each O atom attains an octet
  • the sharing of 2 sets of electrons is a multiple bond called a double bond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

In a nitrogen molecule…

A
  • each N atom shares 3 electrons
  • each N atoms attains an octet
  • the sharing of 3 sets of electrons is a multiple bond called a triple bond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Resonance structure

A
  • 2 or more electron dot formulas for the same arrangement of atoms
  • related by a double - headed arrow
  • written by changing the location of a double bond between the central atom and a different attached atom
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When are prefixes used in nonmenclature for covalent compounds?

A
  • in the names of covalent compounds

- because 2 nonmetals can form two or more different compounds

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

Valence shell electron pair repulsion theory

  • what is it the result of
  • how are they arranged
  • have the least amount of what
  • have what shapes
A
  • the result of bonded groups and lone pairs of electrons around the central carbon atom
  • arranged as far apart from eachother as possible
  • have the least amount of repulsion of the negatively charged electrons
  • have a geometry around the central atom that determines molecular shape
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Trigonal planar

  • example
  • how many electron groups are bonded
  • what happens to repulsion
A
  • BF3
  • 3 electron groups are bonded to the central atom B
  • repulsion is minimized with 3 electron groups at angles of 120
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Bent

  • example
  • how many electron groups are bonded
  • what happens to repulsion
A
  • SO2
  • 2 electron groups bonded to O atoms and one lone pair
  • repulsion is minimized with the electron groups at angles of 120
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Tetrahedral

  • example
  • how many electron groups
  • what happens to repulsion
A
  • CH4
  • 4 electron groups around C
  • repulsion is minimized by placing 4 electron groups at angles of 109
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Trigonal pyramidal

  • example
  • how many electron groups are bonded
  • how many electron groups minimize repulsion
  • degrees
  • what type of arrangement
A
  • H2O
  • 2 electron groups are bonded to H atoms and 2 are lone pairs
  • 4 electron groups
  • 109
  • tetrahedral
17
Q

Polar covalent bonds

  • definition
  • occurs between
  • electronegativity difference
A
  • unequal sharing of electrons
  • nonmetal atoms
  • moderate (0.5-1.7)
18
Q

electronegativity value

  • what does it indicate
  • how does it increase
  • how does it decrease
  • what is it high for
  • what is it low for
A
  • attraction of an atom for shared electrons
  • left to right
  • down a group
  • nonmetals with flourine as the highest
  • metals
19
Q

nonpolar covalent bond

  • what does it occur between
  • equality
  • electronegativity difference
A
  • nonmetals
  • has an equal or almost equal sharing of electrons
  • almost none (0.0-0.4)
20
Q

ionic interaction

  • occurs between
  • result of
  • electronegativity difference
A
  • metal and nonmetal ions
  • electron transfer
  • large (>1.8)
21
Q

nonpolar molecule

  • contains
  • arrangement
A
  • nonpolar bonds

- symmetrical arrangement of polar bonds

22
Q

dipole-dipole attractions

A

exert attractive forces

23
Q

dispersion forces

  • definition
  • caused by
A
  • attractions between nonpolar molecules

- temporary dipoles that develop when electrons are non distributed equally

24
Q

what are the strongest type of dipole-dipole attractions

A

hydrogen bonds because they require more energy to break

25
Q

what are the weakest interactions

A

dispersion forces because they require very little energy needed to change state

26
Q

nuclear chemistry

A

the only subdiscipline of chemistry where the composition of the nucleus changes

27
Q

radioactive isotope

  • type of nucleus
  • omits
  • how many isotopes
A
  • unstable
  • radiation to become more stable
  • can be 1 or more of the isotopes of an element
28
Q

nuclear radiation

A

radiation admitted by an unstable atom

takes the form of alpha particles, neutrons, beta particles, positrons, or gamma rays

29
Q

alpha particle

  • protons and neutrons
  • definition
A

2 protons and 2 neutrons

-heavy and do not travel far

30
Q

beta particle

  • energy
  • mass
  • travel
A

high energy electron

  • less mass
  • farther and through more things
31
Q

positron

A

positive electron

32
Q

gamma ray

  • energy
  • travel
A

high energy released from a nucleus

-through solid objects

33
Q

radiation protection

  • alpha particles
  • beta particles
  • gamma rays
A
  • paper and clothing
  • lab coat or gloves
  • lead shield
  • thick concrete wall
34
Q

nuclear equation

  • represents
  • sums
  • atomic number changes?
  • what will help you know what the new element will be
A
  • nuclear reaction
  • mass and atomic numbers must be equal on both sides
  • elements symbol changes to match
  • type of radiation
35
Q

geiger counter

  • what does it measure
  • detects
  • what does it use
  • units
A
  • radiation
  • beta/gamma
  • ions produced by radiation to create an electrical current
  • curie
36
Q

curie

A

measues activity as the number of atoms that decay in one second

37
Q

radiation absorbed dose

A

measures the radiation absorbed by one gram of body tissue

38
Q

radiation equivalent in humans

  • equation
  • definition
A
  • radxfactor

- measures the biological damage caused by different types of radiation

39
Q

nuclear fission

A

bombardment of a heavy nuclei

Chemistry 101 (7 decks)

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