Brainscape's Knowledge GenomeTM

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


See full index

Gen. Chem. I > Module I > Flashcards

Module I Flashcards

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

Extensive property

A

A property that depends on how much matter you have

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

Intensive property

A

A property that does not depend on its quantity

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

Absolute error =

A

Measured value - True value

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

Relative error =

A

Absolute error / True value

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

What is absolute error?

A

The difference between a measured value and a true value

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

What is relative error?

A

The proportion of the absolute error relative to the measured value

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

Standard state of metals

A

Solid (except for mercury, a liquid)

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

Standard state of nonmetals

A

Solid

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

Standard state of diatomic nonmetals

A

Gas

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

Exceptions to diatomic nonmetal standard states

A

Iodine (solid) and Bromine (liquid)

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

Standard state of phosphorus

A

P4(s)

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

Standard state of sulfur

A

S8(s)

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

Precision

A

How closely clustered together the measurements are

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

Accuracy

A

How close to the true value the measurement is

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

Deuterium

A

Special isotope of hydrogen (1p + 1n)

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

When will charge items not interact?

A

When they are infinitely far apart

17
Q

Quantum number n

A

Principle quantum number, shell number

Roughly describes the distance from the nucleus

Fully describes energy in single electron systems

18
Q

Quantum number L

A

Angular momentum quantum number, subshell

Describes the shape of orbitals

Max value = n-1

19
Q

Quantum number m(L)

A

Magnetic quantum number

Orientation of orbital

-L <= m(L) <= L

20
Q

Quantum number m(S)

A

Spin quantum number

Property of the electron itself, not its orbital

Either +1/2 or -1/2

21
Q

Which electrons are best at screening?

A

The electrons closest to the nucleus are best at screening the nucleus’s charge from outer electrons

22
Q

Why is there no 1p orbital?

A

Because p indicates that L=1, therefore n must equal 2

23
Q

Effective nuclear charge

A

The pull exerted on a specific electron by the nucleus, notated as Z(eff)

24
Q

What makes a group of atoms and/or ions isoelctronic?

A

Sharing the same electron configuration

25
Q

Ionization energy

A

The amount of energy required to remove the most loosely bound electron (cation formation)

26
Q

Electron affinity

A

The energy change for the process of adding an electron to form an anion. Can be endothermic or exothermic.

27
Q

A compound made of nonmetals only is usually…

A

Molecular

28
Q

A compound made of metals and nonmetals is usually…

A

Ionic

29
Q

Natural law definition

A

An observable law relating to natural phenomena

30
Q

Determinate error

A

Causes the mean of a data set to differ from the accepted value

31
Q

Indeterminate error

A

Causes data to be scattered roughly symmetrically around a mean value (also called random error)

32
Q

Dalton’s atomic theory

A
  1. Elements consist of indivisible small particles
  2. All atoms of the same elements are identical
  3. Atoms can neither be created nor destroyed
33
Q

How were electrons discovered?

A

J. J. Thomson’s cathode ray experiments

34
Q

How were nuclei discovered?

A

Rutherford’s gold sheet + alpha particle experiment

35
Q

Bohr’s Atomic Model

A

Electrons revolve around the nucleus in stable orbits without emission of radiant energy. Each orbit has a definite energy and are designated as energy shells or levels

36
Q

Aufbau principle

A

Electrons first fill subshells of the lowest available energy

37
Q

Pauli exclusion principle

A

No two electrons in an atom can have an identical set of four quantum numbers

38
Q

Hund’s rule

A

All orbits will be singly occupied before any is doubly occupied

39
Q

Copper’s electron configuration

A

[Ar] 4s1 3d10

Gen. Chem. I (7 decks)

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