Teas test
Intergers
whole numbers and their opposites no decimals or fractions
Factors and Multiples
FACTORS- factors are the two numbers being multiplied in a multiplication problem. A prime
factorization is when you take a number and break it down into factors over and over until the
last numbers are all prime (only divisible by 1 and itself).
MULTIPLES- Multiples are the result of multiplying a certain number by integers.
Prime numbers
a number which can only be divided by itself and 1 which are:
2,3,4,7,11,13,17,19,23,29,31,37,41,43,47,53,59,61,67,71,73,79,83,87,89,97
prime factorization
First factor the number then find and pull out the numbers that are prime
PEMDAS "Order of Operations"
Please Excuse My Dear Aunt Sally (Parenthesis, Exponents, Multiply, Divide, Add, Subtract);
order in which an equation is worked out - multiplication and division as well as adding and
subtracting can be interchanged, depending on which comes first (from left to right) in the
equation
GCF (Greatest Common Factor)
the greatest number that is a factor of two or more numbers
LCM (Least Common Multiple)
,The smallest whole number greater than 0 that is a common multiple of each of two or more
numbers.
Rules if exponents
Must always share a base
1. When multiplying you add the exponents
2. When diving you subtracts the exponents
3. A number raised to a fraction power is the same as the root or radical
perfect square
These are 1,4,9,25,36,49,64,81,100
Factorials (e.g. 8!)
To find the factorial of any integer, multiply it by every positive integer below it, e.g.:
8x7x6x5x4x3x2x1
Quadratic Formula
x = -b ± √(b² - 4ac)/2a
Foil
First, Outside, Inside, Last
physical properties of matter
Color, Odor, Shape, Hardness, Texture, Density, Volume, Mass, Weight
Mass
A measure of the amount of matter in an object ( sum of the protons, neutrons, and electrons)
mass of proton
1.67 x 10^-27 kg equal to 1.007 amu
Weight
A measure of the gravitational force exerted on an object.
Volume
The amount of space an object takes up
,Density
Mass per unit volume (equals mass/volume)
What's the smallest unit of matter
Atom
atomic weight/mass
protons + neutrons
Ions
positively and negatively charged atoms
anions and cations
- Anions: negatively charged ions
- Cations: positively charged ions
Isotopes
Atoms with the same number of protons but different numbers of neutrons
atomic weight
Average of the mass numbers of all isotopes (usually 2x the atomic number)
The atomic nucleus
The central part of an atom that contains both protons and neutrons.
Atomic Energy States
All atoms strive to thrive lowest energy state
The N shells
Energy levels where the electrons are found, the lowest energy leve
Orbitals/Shells
regions around the nucleus in which given electron or electron pair is likely to be found ex) 1s
which can only hold 2 electrons
p orbital
6 electrons
, electron configuration
the arrangement of electrons of an atom in its ground state into various orbitals around the
nuclei of atoms ex) N= 1s2, 2s2, 2p3
valance electrons
electrons in the outermost energy level These participate in chemical reactions
The octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence
electrons
Transition Metals (Groups 3-12)
good thermal conductors, shiny, electric conductors, higher density and melting points than
group and low specific heat, and can be shapes and stretched
Nonmetals
These are carbon, nitrogen , oxygen, phosphorus, sulfur and the halides form small molecules,
strong covalent bonds and weak intermolecular attractions , brittle and powdery, good electrical
and thermal insulators
metalloids physical properties
brittle, can be shiny or dull, can be ductile or malleable, used as semiconductors in electronics
ex) silicon and germanium
Ionic bonds form between
metals and nonmetals
Hydrogen bonds are
strongest intermolecular forces
covalent bond
a bond formed when atoms share one or more pairs of electrons
polar bonds are
unequal sharing, hydrophilic, they do not dissolve in water
intermolecular forces
forces of attraction between molecules ex) soild, gas , liquid these are weak
Intergers
whole numbers and their opposites no decimals or fractions
Factors and Multiples
FACTORS- factors are the two numbers being multiplied in a multiplication problem. A prime
factorization is when you take a number and break it down into factors over and over until the
last numbers are all prime (only divisible by 1 and itself).
MULTIPLES- Multiples are the result of multiplying a certain number by integers.
Prime numbers
a number which can only be divided by itself and 1 which are:
2,3,4,7,11,13,17,19,23,29,31,37,41,43,47,53,59,61,67,71,73,79,83,87,89,97
prime factorization
First factor the number then find and pull out the numbers that are prime
PEMDAS "Order of Operations"
Please Excuse My Dear Aunt Sally (Parenthesis, Exponents, Multiply, Divide, Add, Subtract);
order in which an equation is worked out - multiplication and division as well as adding and
subtracting can be interchanged, depending on which comes first (from left to right) in the
equation
GCF (Greatest Common Factor)
the greatest number that is a factor of two or more numbers
LCM (Least Common Multiple)
,The smallest whole number greater than 0 that is a common multiple of each of two or more
numbers.
Rules if exponents
Must always share a base
1. When multiplying you add the exponents
2. When diving you subtracts the exponents
3. A number raised to a fraction power is the same as the root or radical
perfect square
These are 1,4,9,25,36,49,64,81,100
Factorials (e.g. 8!)
To find the factorial of any integer, multiply it by every positive integer below it, e.g.:
8x7x6x5x4x3x2x1
Quadratic Formula
x = -b ± √(b² - 4ac)/2a
Foil
First, Outside, Inside, Last
physical properties of matter
Color, Odor, Shape, Hardness, Texture, Density, Volume, Mass, Weight
Mass
A measure of the amount of matter in an object ( sum of the protons, neutrons, and electrons)
mass of proton
1.67 x 10^-27 kg equal to 1.007 amu
Weight
A measure of the gravitational force exerted on an object.
Volume
The amount of space an object takes up
,Density
Mass per unit volume (equals mass/volume)
What's the smallest unit of matter
Atom
atomic weight/mass
protons + neutrons
Ions
positively and negatively charged atoms
anions and cations
- Anions: negatively charged ions
- Cations: positively charged ions
Isotopes
Atoms with the same number of protons but different numbers of neutrons
atomic weight
Average of the mass numbers of all isotopes (usually 2x the atomic number)
The atomic nucleus
The central part of an atom that contains both protons and neutrons.
Atomic Energy States
All atoms strive to thrive lowest energy state
The N shells
Energy levels where the electrons are found, the lowest energy leve
Orbitals/Shells
regions around the nucleus in which given electron or electron pair is likely to be found ex) 1s
which can only hold 2 electrons
p orbital
6 electrons
, electron configuration
the arrangement of electrons of an atom in its ground state into various orbitals around the
nuclei of atoms ex) N= 1s2, 2s2, 2p3
valance electrons
electrons in the outermost energy level These participate in chemical reactions
The octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence
electrons
Transition Metals (Groups 3-12)
good thermal conductors, shiny, electric conductors, higher density and melting points than
group and low specific heat, and can be shapes and stretched
Nonmetals
These are carbon, nitrogen , oxygen, phosphorus, sulfur and the halides form small molecules,
strong covalent bonds and weak intermolecular attractions , brittle and powdery, good electrical
and thermal insulators
metalloids physical properties
brittle, can be shiny or dull, can be ductile or malleable, used as semiconductors in electronics
ex) silicon and germanium
Ionic bonds form between
metals and nonmetals
Hydrogen bonds are
strongest intermolecular forces
covalent bond
a bond formed when atoms share one or more pairs of electrons
polar bonds are
unequal sharing, hydrophilic, they do not dissolve in water
intermolecular forces
forces of attraction between molecules ex) soild, gas , liquid these are weak
