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