Chemistry - Atomic Structure (Ch 1 formulas)

shape of d orbital

four-leaf clover

last line has max ____ and min ____

frequency, wavelength

third line of any series

gamma series

phosphorescent

giving off light without heat

greater the value of principal quantum number

greater is the distance of nucleus and energy of the shell

final kinetic energy

initial potential energy

Drawbacks of Rutherford's Model

it could not explain the stability of an atom. if electrons lose energy continuously the spectrum would be continuous but it consists of well defined lines of definite frequencies.

Heisenberg uncertainty principle

it is impossible to know exactly both the velocity and the position of a particle at the same time

charge is quantised

minimum amount of chaege a body can have is +/- 1.6*10^-19 C .

seperation energy

minimum energy needed to move an atom from its excited state

isosters

molecules with same number of atoms and electrons

second postulate on which Bohr's atomic model is based on

negatively charged electron revolve around the nucleus in the same way the planets revolve around the sun. the path of electron is circular. the attraction force between nucleus and electron is equal to the centrifugal force on electron.

frequency of wave

number of complete waves that pass a point per second

smallest packet of energy of light

photon

if the value of n is same then the oder of energy of the various subshells will be

s<p<d<f (only for multi electron species)

isotones/isoneutronic species/isotonic

same number of neutrons, different number of protons

isobars don't have

same physical and chemical property

isotopes do not have

same value of e/m

bohr model is applicable only for

single electron species

total energy transmitted from one body to another will be

some integral multiple of energy of a quantum

quantum numbers

specify the properties of atomic orbitals and the properties of electrons in orbitals

frequency equals

speed of light/wavelength

shape of s orbital

sphere

magnetic quantum number (m)

symbolized by m, indicates the orientation of an orbital around the nucleus

principal quantum number (n)

symbolized by n, indicates the main energy level occupied by the electron

radius of the nucleus is proportional to

the cube root of the number of nucleons within it.

Hydrogen Line Spectrum

the em spectrum of hydrogen.

sixth postulate on which Bohr's atomic model is based on

the emission or absorption of energy in the photon can only occur when electron jumps from one stationery state to another. energy is absorbed when electron jumps from inner to outer orbit and is emitted when electron moves from out to inner orbit.

excitation energy

the energy required to move an electron from a lower energy level to a higher energy level

Ionisation energy

the energy required to remove an electron from an atom

Amplitude

the height of a wave's crest

bohr's theory and de-broglie concept

the nature of an electron moving around the nucleus is like a wave that flows in circular obits around the nucleus. if an electron is regarded as a wave, the quantum condition as given by Bohr in his theory is readily fulfilled.

Atomic number of an element (Z)

the number of protons in each atom of the element

fourth postulate on which Bohr's atomic model is based on

the orbits in which electron can revolve are known as stationary orbits because in these orbits energy of electron is always consistent.

electromagnetic spectrum

the range of wavelengths or frequencies over which electromagnetic radiation extends.

mass number (A)

the total number of protons and neutrons in the nucleus of an atom

Properties of cathode rays

they move in a straight line particles of cathode ray have mass particles are made of -ve particles amount of deflection is proportional to charge/mass charge/mass ratio remains constant.

first line has max _____ and min ____

wavelength, frequency

radial nodes

}|+ +

charge of a electron

-1.6 x 10^-19 C

final potential energy

0

initial kinetic energy

0

value of l lies between

0 to n-1 in a particular shell

Dalton's Atomic Theory

1) elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together 4) atoms only change when mixed with other elements

Charge of a proton

1.6 x 10^-19 C

e/m value constant

1.7*10^11 C/Kg

kinetic energy

1/2 mv^2

time period of wave

1/frequency

if value of l is same but value of n is different then the order of energy will be

1s<2s<3s<4s<5s<6s, 3d<4d<5d<6d, 4p<5p<6p

radius of an atom

1x10^-10m

radius of nucleus

1x10^-15

the number of electrons in a particular subshell is equal to

2(2l +1)

charge of alpha particle

3.2 * 10^-19 C

Distance of closest approach

4ZKe^2/mv^2

Planck's constant (h)

6.626 x 10^-34

orbital

A 3D region around the nucleus that indicates the probable location of an electron.

electromagnetic waves

A form of energy that can move through the vacuum of space.

Lyman series

A set of spectral lines that appear in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.

Balmer series

A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.

Paschen series

Set of spectral lines resulting when a hydrogen atom undergoes a transition from energy levels n>3 to n=3.

Brackett Series

Set of spectral lines resulting when a hydrogen atom undergoes a transition from energy levels n>4 to n=4.

Pfund Series

Set of spectral lines resulting when a hydrogen atom undergoes a transition from energy levels n>5 to n=5.

humphrey series

Set of spectral lines resulting when a hydrogen atom undergoes a transition from energy levels n>6 to n=6.

isoelectric species

atoms and ions that have the same number of electrons in their outer shell

first postulate on which Bohr's atomic model is based on

atoms has a nucleus where all protons and neutrons are present. the size of nucleus is very small and it is present at the centre of the atom.

wave number

The number of waves per centimeter.

spin quantum number (s)

The quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital

isodiaphers

atoms of different element which have same difference of the number between neutrons and protons

isobars

atoms of different elements with same mass number but different atomic number.

second line of any series

beta series

Values of a principal quantum number?

between 1 and infinity

shape of f orbital

complex

wave mechanical model of atom

consists of de-Broglie concept and Heisenberg's Uncertainty Principle

Millikan's Oil Drop Experiment

determined the charge of the electron in an oil drop

energy of each quantum is

directly proportional to the frequency of the radiation

shape of p orbital

dumbbell

fifth postulate on which Bohr's atomic model is based on

each stationary orbit is associated with definite amount of energy therefore these orbits are also called energy levels

mass of _____ is less than that of hydrogen.

electron

third postulate on which Bohr's atomic model is based on

electrons can revolve only in these orbits in which angular momentum of electron is integral multiple of h/2pi.

classification of spectrum

emission spectrum and absorption spectrum

Planck's Quantum Theory

energy emitted as electromagnetic radiation from matter exists in discrete bundles called quanta

cathode tube experiment

experiment done by JJ Thomson in which he discovered the electron

azimuthal quantum number (l)

Second quantum number, designated l. Tells us the shapes of the electron orbitals

Bohr's Atomic Model

Atoms have levels surrounding the nucleus where electrons are found. Levels can hold different amounts of electrons depending on their distance from the nucleus.

isotopes

Atoms of the same element that have different numbers of neutrons

atomic weight

Average of the mass numbers of all isotopes

Coloumb's Law

F=kq1q2/r^2

Wavelength

Horizontal distance between the crests or between the troughs of two adjacent waves (lambda)

Neutrons were discovered by

James Chadwick in 1932

initial potential energy

K(2e)(Ze)/r

potential energy of charge q1 due to charge q2

Kq1q2/r

JJ Thomson's atomic model

Plum pudding model

when an electric excitation is applied on hydrogen atomic gas at low pressure,

a bluish light is emitted. when it is passed through prism, a spectrum of several isolated sharp lines is obtained.

node

a point, line, surface or plane in which probability of finding an electron is maximum

the dual nature of matter

according to de-Broglie, if the nature of light is both that of a particle of a wave, then this dual behaviour should be true also for the matter

value of magnetic quantum number

all integral value from -l to l including 0

first line of any series

alpha series