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ATI -TEAS Practice Exams
Finals
Ch.2- Basic Chemistry
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ATI -TEAS Practice Exams > Finals > Ch.2- Basic Chemistry
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ATI -TEAS Practice Exams > Finals > Ch.2- Basic Chemistry
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Matter
-Anything that has
mass
and takes up
space
(weight)
- Solids,
Liquids
, and
Gasses
-
Physical
&
Chemical
changes
Energy
the
ability
to do
work
Kinetic
energy
when energy is actually doing work
Potential
Energy (PE)
When energy is
inactive
or
stored
Forms of Energy
chemical,
electrical
, mechanical,
radiant
Chemical
energy
stored in
bonds
of chemical substances
Electrical
energy
results from the
movement
of
charged
particles-ions
Mechanical
energy
directly involved in moving
matter- muscles
Radiant
energy
travels in waves- the electromagnetic spectrum including x-rays, infrared, light, radio, and UV rays
Fundamental units of
matter
can't be
broken down
into
smaller
units
96% of the body is made from 4 elements
Carbon (C),
Oxygen
(O), Hydrogen (H),
Nitrogen
(N)
Atoms
building blocks of
elements
Inside the nucleus
protons
and
neutrons
Outside the nucleus
electrons
Atomic
number
equal to the number of
protons
that the atoms contain - also equals the number of
electrons
Atomic
Mass Number (amu)
Sum of
protons
and
neutrons
Isotopes
-Have the same number of
protons
and
electrons
, but the same atomic number
- Vary in number of
neutrons
so different
atomic
masses
Atomic
weight
-close to
mass number
of most
abundant
isotope
-atomic weight reflects
natural
isotope variation
Radioisotopes
-Heavy
isotope
- Tends to be
unstable
- Decomposes to move
stable
isotope
Radioactivity
- process of
spontaneous
atomic
decay
- releases particles (alpha,
beta
, and
gamma
rays)
Molecule
2
or
more
atoms
combined chemically
Compound
2
or
more
DIFFERENT
atoms combined chemically
Chemical
Reactions
Occurs when
atoms
combine or
dissociate
from other atoms
In chemical reactions, atoms are
-united by
chemical
bonds
-dissociated
from other atoms when chemical bonds are
broken
Electrons
-Negatively
charged
particles
- occupy
energy levels
called
electron levels
or shells
-
closest
to the
nucleus
and most strongly attracted
Each
shell has distinct
properties
-The number of
electrons
has an upper
limit
-Shells
closest
to the nucleus fill first
Bonding
Involves interactions between electrons in the
outer shell
(Valence shell)
Full
valence shells do not form
bonds
Inert elements
have complete
valence
shells and are
stable
Rules of 8s
Step 1: Shell 1 has
2
Step 2: Shell 2 has
10
electrons
Step 3: Shell 3 has
18
electrons
Reactive
Elements
-valence shells are not
full
and are
unstable
-tend to gain,
lose
, or
share
electrons
-allows for
bond formation
, which produces
stable
valence
Ionic
bonds
form when
electrons
are completely transferred from
one
atom
to
another
Ions
-charged
particles
- either
donate
or
accept
electrons
Anions
negatively
charged ions (accept electrons)
Cations
positively
charged ions (
donate
electrons)
Opposites
attract so stick together
most
form salts
Covalent
Bonds
-atoms become
stable
through
shared
electrons
-
Single
covalent bonds share
one
electron
-
Double
covalent bonds share
two
electrons
Covalent bonded molecules
-some are
non-polar
:
electrically neutral
as a molecule
-some are
polar
: have a
positive
and
negative side
Polar molecules orient themselves toward other
polar
or
charged
particles
Hydrogen
bonds
-weak
chemical bonds
-hydrogen is attracted to the
negative
portion of
polar
molecule
-provides attraction between
molecules
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