Download Matter – Chemical and Physical Properties

Science Prep Course
Study Guide for Exam 2
Matter – Chemical and Physical Properties
atom – smallest particle of an element that has all of the element’s chemical properties
Brownian motion – haphazard movement of tiny particles suspended in a gas or liquid
resulting from bombardment by the fast-moving molecules of the gas or liquid
molecule – smallest particle of any substance that has all the substance’s chemical
properties
chemical reaction – process of rearrangement of atoms transforming one molecule into
another
Avogadro’s principle – equal volumes of all gases at the same temperature and pressure
contain the same number of molecules
atomic mass unit (amu) – standard unit of atomic mass (based on mass of Carbon
(Carbon = 12 amu exactly))
compound – chemical substance made of atoms of two or more different elements
combined in a fixed proportion
mixtures – substances mixed together without combining chemically
atomic number – number of protons in the nucleus of an atom
periodic table – chart listing elements by atomic number and electron arrangements so
that elements with similar chemical properties are in the same column
antimatter – matter composed of atoms with negative nuclei and positive particles
orbiting in shells
Particle
Antiparticle
Proton
Antiproton
Neutron
Antineutron
Electron
Positron
plasma – fourth phase of matter which consists of positive ions and free electrons. Most
of the matter in the universe is in the plasma phase
atomic bonding – linking together of atoms to form larger structures, including solids
Types of Bonds
Covalent bond – one or more electrons are shared between two atoms
Ionic bond – one or more electrons are transferred from one atom to another
Metallic bond – described as a “sea of electrons”. Electrons move from atom to atom
freely (this causes metals to be excellent conductors)
James bond – Agent 007, subject of many movies
density – mass per unit volume (REMEMBER: “Per” means “divided by”!!!!!) d=m/v
elasticity – property of a material wherein it changes shape when a deforming force acts
on it and returns to its original shape when the force is removed
Hooke’s law – amount of stretch or compression of an elastic material is directly
proportional to the applied force (EXAMPLE: If a 10 N force stretches a spring 5 in.,
then a 20 N force will stretch the spring 10 in. and a 5 N force will stretch it 2.5 in.)
scaling – study of how size affects the relationships among weight, strength, and surface
pressure – ratio of force to the area over which that force is distributed (pressure =
F/area)
buoyant force – net upward force that a fluid exerts on an immersed object
Archimedes’ principle – an immersed body is buoyed up by a force equal to the weight
of the fluid it displaces
Pascal’s principle – pressure applied to a motionless fluid in a container is transmitted
undiminished throughout the fluid
surface tension – tendency of the surface of a liquid to contract in area and thus behave
like a stretched elastic membrane
capillary action – rise of a liquid in a fine, hollow tube or in a narrow space
meniscus – due to capillary action, liquid in a tube (usually glass) is U-shaped on the top.
The meniscus is the point at the bottom of the u where measurement should be read from
atmospheric pressure – pressure exerted against bodies immersed in the atmosphere
resulting from the weight of air pressing down from above
barometer – device that measures atmospheric pressure
Boyle’s law – at a constant temperature, an increase in pressure causes a decrease in the
volume of a gas and a decrease in pressure causes an increase in volume of a gas
P1V1=P2V2
Charles’ law – at a constant pressure, an increase in temperature causes an increase in
the volume of a gas and a decrease in temperature causes a decrease in volume of a gas
P1 P2
--- = --T1 T2
Bernoulli’s principle – the pressure in a fluid moving steadily decreases when the fluid’s
velocity increases