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Chemistry > Atomic and molecular structure > Flashcards

Atomic and molecular structure Flashcards

1
Q

Atom

A

Basic building block of matter representing the smallest unit of a chemical element. Composed of some atomic particles protons, neutrons and electrons. Nucleus at the core containing protons and neutrons. Electrons in regions of space called orbitals

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2
Q

Dalton’s atomic theory

A
  • All elements are composed of very small particles called Adams. All Adams of an element are identical in size, mass, chemical properties
  • All compounds are composed of atoms of more than one element
  • A chemical reaction Involves the separation, combination, or rearrangement of atoms. It does not result in the creation or destruction of atoms
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3
Q

Proton

A 
Positive charge
1 amu = 1 Da
Atomic number (Z)
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4
Q

Neutron

A

No charge

1 amu

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5
Q

Isotopes

A

One element which has different numbers of neutrons but the same number of protons

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6
Q

Electron

A

Negative charge

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7
Q

Valence electrons

A

Electrons in the electron shell farthest from the nucleus. Have weaker attractive force of the positively charged nucleus

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8
Q

Ion

A

A positive or negative charge on an atom due to the loss or gain of electrons

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9
Q

Atomic number (Z)

A

The number of protons/electrons in a neutral atom

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10
Q

Mass numbers (A)

A

The total number of protons and neutrons

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11
Q

Molecular weight

A

The weight in grams per one mole of a given element

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12
Q

Mole

A

A unit used to count particles

Represented by Avogadro’s number

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13
Q

Avogadro’s number

A

6.02 x10^23

How many atoms of carbon are in 12 g of carbon-12

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14
Q

Standard atomic weight

A

A weighted average of all the isotopes of an element found naturally on earth

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15
Q

Quantum theory

A

Max Planck
Energy admitted as electromagnetic radiation from matters comes in discreet bundles called quanta
E = hf

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16
Q

Planck’s constant (h)

A

6.626 x 10^-34 Js

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17
Q

Bohr Model

A

An electron can exist only in certain fixed-energy states. A central proton around which electrons travel in a circular orbit and be centripetal force acting on the electron is the electrical force between positively charged protons and negatively charged electrons

18
Q

Ground state

A

The lowest energy state of an electron

19
Q

Atomic emission spectrum

A

The line spectrum of light at specific frequencies where each line on the emission spectrum corresponds to a specific electronic transition. Unique for each element

20
Q

Baller series

A

Transition from n>2 to n=2

Visible and ultraviolet

21
Q

Lyman series

A

Transition from n>1 to n=1

Ultraviolet

22
Q

Paschen series

A

Transition from n>3 to n=3

Infrared

23
Q

Atomic absorption spectrum

A

The expectation of electrons in a particular element results in energy absorptions at specific wavelengths. Wavelength of absorption correspond directly to wavelengths of the Mission

24
Q

Heisenberg uncertainty principle

A

It is impossible to simultaneously determine with perfect accuracy the momentum in the position of an electron

25
Q

Orbitals

A

A representation of the probability of finding an electron within a given region. A specific region with in a sub shell that may contain no more than two electrons

26
Q

Pauli exclusion principle

A

No two electrons in a given atom can possess the same set of four quantum numbers

27
Q

Energy state

A

The position an energy of an electron described by its quantum numbers

28
Q

Principal quantum number, n

A

The shell where an electron is present in an atom

29
Q

Azimuthal quantum number, l

A

Angular momentum quantum number
The subshells or sublevels that occur within each principal energy level
0 to n-1

30
Q

4l+2

A

The maximum number of electrons that can exist within a sub shell

31
Q

Magnetic quantum number, ml

A

The orientation of the orbital in space

l to -l

32
Q

2n^2

A

The maximum number of electrons in an electron shell

33
Q

Spin quantum number, ms

A

Intrinsic angular momentum

1/2 and -1/2

34
Q

Parallel spins

A

Same ms value

35
Q

Paired spins

A

Different ms values

36
Q

Electron configuration

A

The pattern by which subshells are filled and the number of electrons within each principal level and some shell are designated

37
Q

Aufbau principle

A

Subshells are filled from lowest to highest energy

38
Q

n+l rule

A

The lower the sum of the first and second quantum numbers, the lower the energy of the sub shell

39
Q

Hund’s rule

A

Within a given some shell, orbitals are filled such that there are a max number of half filled orbitals with parallel spins

40
Q

Paramagnetic

A

Unpaired electrons. A magnetic field will align the spins of these electrons in weekly attract the atom to the field

41
Q

Diamagnetic

A

No unpaired electrons. Are slightly repelled by a magnetic field

Chemistry (15 decks)

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