Chem CH 2
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| The Periodic Table created by | Late 1800's by Mendeleev (during dream)
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| Elements represented by | Chemical Symbols: 1-3 letters; 1st letter is capitalized
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| Elements are divided into 3 groups | - metals
- metalloids
- nonmetals
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| Metals | left side of PT
shiny, malleable, ductile
good conductors of electricity
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| Nonmetals | right side of PT
dull
poor conductors
opposite of metals
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| Metalloids | along zigzag lines
properties of metals & nonmetals
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| What are the building blocks of life? | Oxygen
Carbon
Hydrogen
Nitrogen
all four are nonmetals
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| How much mass of human body does the building blocks of life take up? | 96%
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| Periodic Law | properties repeat themselves when elements are arranged in orders of increasing Atomic #
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| Family/Groups | vertical columns
1A-8A
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| Period | horizontal row
numbered
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| Special Groups of Elements | - Alkali Metals
- Alkaline Earth Metals
- Transition Metals
- Halogen
- Noble Gases
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| Alkali Metals | 1A
Vert Reactive
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| Alkaline Earth Metals | 2A
Reactive
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| Transition Metals | "B" Block
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| Halogen | 7A
Diatonic Elements
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| Noble Gases | 8A
Stable
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| Who came up with structure of the atom? | John Dalton
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| All matter is made up of particles called? | atoms
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| All atoms of the same element are ______________ & ______________atoms of other elements | identical to one another; different from
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| ____________ of 2+ elements combined to form __________ | atoms; compounds
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| A ___________ ___________ involves the rearrangement of __________ | chemical reaction; atoms
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| Subatomic Particles | - Protons
- Neurons
- Electrons
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| Protons | p+
1
positive charge
inside nucleus
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| Neutron | N
1
neutral charge
inside nucleus
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| Electron | E-
1/1840
negative charge
on electron cloud
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| Atoms have what type of charge? | electrically neutral b/c protons & electrons cancel each other out
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| Atomic # made up of ? | protons and electrons
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| each atom has its own | atomic number
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| Mass # is made up of | protons and Neutrons
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| Mass # must be a _________ __________ | whole number
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| In an isotope symbol ___________ ___________ is on top & _________ _____________ is on bottom | Mass Number; Atomic Number
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| Isotope | atoms of the same element that have a different # of Neutrons
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| Atomic Mass / Weight | the "average atom" of each element
the weighted average mass of all naturally occurring isotopes
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| Atomic Mass/AMU has how many sigfigs | 4 sigfigs
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| Electrons are confined to ________ ( _________ _____ / ______) | energy; energy shells; levels
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| Electrons can shift to __________ _________ & emit _________ ( _______________) | excited states; emit light; energy
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| ground state | when electrons have the lowest energy
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| electrons of similar energy are grouped into? | Shells (labeled 'n')
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| Shell 1 holds | 2 electrons
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| Shell 2 holds | 8 electrons
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| Shell 3 holds | 18 electrons
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| Shell 4 holds | 32 electrons
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| Shell 1 has how many subshells | 1 subshell
1s
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| Shell 2 has how many subshells | 2 subshells
2s, 2p
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| Shell 3 has how many subshells | 3 subshells
3s, 3p, 3d
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| Shell 4 has how many subshells | 4 subshells
4s, 4p, 4d, 4f
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| each subshell has ___________ | orbitals
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| orbitals | particular shaped space that holds 1 to 2 electrons
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| S subshell has _________ & holds ___________ | 1 orbital; 2 electrons
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| P subshell has _________ & holds ___________ | 3 orbitals; 6 electrons
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| D subshell has __________& holds ___________ | 5 orbitals; 10 electrons
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| F subshell has __________ & holds _________ | 7 orbitals; 14 electrons
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| Pacli exclusion principles | 2 electrons in an orbital have opposite spins
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| Electron configuration & arrangement | describes/defines the organization of electrons
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| Electron Configuration address | look at notes
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| Electron Arrangement | draw a picture showing protons, neutrons, and electrons in shells, subshells, orbitals
look at notes
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| Electron Configuration superscripts represents ________ ___ _________ in each element | number of electrons
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| Noble Gas Notation | shorthand configuration
uses the electron configuration of the noble gas
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| what does Noble Gas Notation look like? | Na = (Ne) 3e1
square brackets
uses noble gas before it
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| Valenic Electrons | outermost occupied shell highest energy
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| Group # = ________________________ | # of valence electrons
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| Electron Dot Symbol | used to represent valance electrons
don't pair until you have too
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| Electron Dot Symbol is also know as? | Lewis Dot Structure
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| Atomic Size | measured by atomic radius
(distance from nucleus to outer edge of valence shell)
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| Atomic Size __________ down a group & going across a row | increases (more layers of electrons)
decreases (as the # of protons in nucleus increases)
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| Ionization Energy | the energy required to remover an electron from an atom
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| Ionization Energy _________ going down a group & ___________ from left to right across a period as the protons inreases | decreases (electrons further from nucleus)
increases
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| atom | the basic building block of matter composed of a nucleus and an electron cloud
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| Periodic Table | groups of elements have similar properties and these elements could be arranged in a schematic way
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| Carbon, hydrogen, and oxygen are found in 4 types of biological moecules | proteins
carbohydrates
lipids
nucleic acids
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| Major Minerals | Macronutrients
one of the seven elements present in the body in small amounts
Potassium
Magnesium
Calcium
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| Trace Elements | Micronutrients
an element required in the daily diet in small quanties
less than 15 mg
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| chemical formula | uses element symbols to show the identity of the elements forming a compound and subscripts to show the ratio of atoms contained in the compound
ex. H2O
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| all matter is composed of the same basic building blocks called? | atoms
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| Nucleus | dense core containing protons and neutrons
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| most of the mass of an atom resides in the> | nucleus
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| Electron cloud | composed of electrons that move rapidly in the almost empty space surrounding the nucleus
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| the electron cloud comprises most of the ______ of an atom | volume
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| Atomic Mass Unit | defines the mass of individual atoms relative to a standard mass
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| Atomic # | is the # of protons in the nucleus
in periodic table it is the # above element
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| Mass # | Protons + Neutrons
in periodic table it is the # below element
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| Atomic Weight | atomic mass
weighted average of the mass of the naturally occurring isotopes of a particular element reported in the atomic mass units (AMU)
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| Lanthanides | a group of 14 elements in the periodic table that begin with Z and immediately following the element La
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| Actindies | a group of elements that begin with Z + 90 following element Ac
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| elements that comprise a particular group have _________________________. | similar chemical properties
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| Alkali metals characteristics | soft
shiny
low melting points
good conductors of heat and electricity
react readily with water to from basic solutions
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| Noble Gases are | stable
rarely combine with other elements to form compounds
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| In their element form, halogens contain ____________. | 2 atoms joined together
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| Diamond | hard because it contains a dense 3-d network of carbon atom sin a six-membered rings
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| Graphite | a slippery black substance used as a lubricant
used in pencils
the softest of carbons
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| the chemical properties of an element are determined by the # of ________ in the atom | electrons
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| Electrons do not move _______ in space. confined to _______ _______. giving it a ________ ________ | freely
specific region
particular engery
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| Electrons occupy discrete _______ _________. | energy levels
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| The energy of electrons is | quantized
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| quantized means | the energy is restricted to specific values
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| the farther a shell is from the nucleus, the ______ its volume becomes, & the ______ electrons it can hold | larger
more
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| electrons closer to the nucleus are held _____ _______ and are _________ in energy | more tightly
lower
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| Electrons farther from the nucleus are held ______ _____ and are ________ in energy | less tightly
higher
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| orbital | a region of space where the probability of finding an electron is high
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| each orbital holds how many electrons | 2
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| why would a s orbital have lower energy than another orbital in the same shelf | because the electrons are kept closer to the nucleus
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| why would a p orbital have more energy than that of a s orbital in the same shelf | because the electrons are further from the nucleus
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| ground state | the lowest energy arrangement of electrons
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| electron configuration | how the electrons are arranged in an atom's orbital
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| orbital diagrams |
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| unpaired electron | a single electron
shown with a single arrow pointing up
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| paired spins | 2 electrons in an orbital
spins are opposite
shown as up and down arrows
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| atomic # tells us_____ | how many electrons must be place in orbitals
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| valence shell | the outermost shell
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| valence electrons | electrons in the outermost shell
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| Elements in the same group have the _______ _____ of valence electrons and _____ _______ | same # of valence electrons
similar electronic configurations
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| the group number equals the ______ ____ ____ _____ for main group elements | number of valence electrons
ex. alkali metals in group 1A have 1 valence electron
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| periodic trends | they change in a regular way across a row or down a column
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| Atomic Size | the size of an atom is measured by its atomic radius
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| atomic radius | the distance from the nucleus to the outer edge of the valence shell
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| The size of atoms ______ down a column of the periodic table, as the ________ _____ are father from the nucleus | increases
valence electrons
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| the size of atoms _____ across a row of the periodic table as the number of protons __________. | decreases
increases
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| An _______ # of protons pulls the electrons _______ to the nucleus, so the atom gets ___________ | increasing
closer
smaller
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| ionization energy | is the energy needed to remove an electron from a neutral atom
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| cation | positively charged
has fewer electrons than the neutral atom
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| Ionization energies ______ ______ a column of the periodic table as the ________ _________ get farther from the postively charged nucleus. | decreases down
valence electrons
farther
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| Ionization energies generally __________ across of the table as the number of protons in the nucleus _________ | increases
increases
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| Ionization Energy increases as you...... | go diagonally up (from left to right across periodic table)
more energy is required to remove electron because of fewer shells; nucleus acts a gravity, has stronger hold on electrons
start from Fr go diagonally up to F
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| this group is not included in ionization energy | noble gases
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| Atomic Size increases as you | go diagonally down (from right to left across the period table)
everything is getting pulled way from nucleus due to increase of valence shells
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