Kinetic molecular Flashcards
states of matter
solid liquid gas
Brownian
random movement of particles
diffusion particles move from high concentration to low
solid
occupies constant amount of space
define space and volume
held by fixed lattice
strong force of attraction
lattice
arrangement of participles in a regular pattern
liquid
occupies a constant amount of space
force of attraction weak particles freedom to move
gas
occupies definite amount of space and volume
small force of attraction move freely
freezing
temp at which a liquid becomes a solid
melting
temp at which a solid becomes a liquid
boiling
How does it change
temp at which a liquid becomes a gas
boiling point changes depending on atmosphere pressure changes w/ attitude
evaporation
any temp
occurs on surface of liquid
no bubbles
condensation
liquid formed from gas
opposite of evaporate
gas particles lose energy
no energy to stay gas
sublimation
solid change to gas
substances with wear forces of attraction
kinetic molecular theory
the force between molecules and the kinetic energy between them. particulates are in constant motion also forces of attraction strong between solid weak by gas
assumptions
matter composed of small particles
particles are in constant motion
solid molecule
vibration
strong force of attraction
least amount of kinetic energy
liquid mole
flow over anther
moderate force of attraction
more kinetic energy
gas mole
continue in straight line
kinetic energy stronger than attraction force
Rutherford gold foil experiment
positive nucleus in center of atom
stuck thin sheets of gold foil w/alpha particles
alpha particles
pass through between positive nuclei
deflected -close to nucleus
hit nucleus head on
atom mass diameter
size depends on number of protons neutrons and electrons
No.of protons in nuc
= atomic No.
atomic No.
= above symbol
mass No.
pro + neutrons (nucleus)
isotopes
atoms that have the same atomic No. but different mass No. No. of protons cant change but No. of neutrons can change
flame test
identify metal of action
flame color
position
arranged in increase atomic No.
valance indicated top column
electrons in outer energy level
group No. indicates No. of valance electrons
row
energy level
size of an atom
distance from nuc to boundary
top to bottom
radius increase No. of electrons increase
atomic radius (up) energy levels (up)
left to right
atomic radi dec bcz same energy level
No. protons increase force of attraction are stronger
electrons are closer to nucleus
density of element
how many atoms are found in volume left to right increase metals decrease through non metals metals high density
top to bottom
increase
atomic radi and volume increase
atoms get bigger cant pack more in same space as smaller atoms
ionization energy of element
amount of energy to remove an element from neutral atom
indicate strength of atoms holding on to its electrons
top to bottom
ionization energy decrease
electrons are further away from nucleus
atomic radius increase
left to right
ionization energy increase
atomic radi decrease
difficult to break particles
