Intro to Chemistry – Flashcards
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| Vertical columns are called |
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| groups |
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| Groups contain elements with |
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| similar properties in vertical columns |
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| Horizontal rows of elements |
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| are periods |
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| Groups are number from |
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| 1-18 or 1A-8A in earlier systems |
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| Periods are numbered from |
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| 1-7 |
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| Period 1 has how many elements |
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| 2 |
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| Period 2&3 have how many elements |
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| 8 |
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| Period 4&5 have how many elements |
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| 18 |
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| Period 6 has how many elements |
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| 32 |
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| A group's special name |
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| main group/Representative elements |
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| B Group's special name |
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| transition elements |
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| Alkali Metals are in Group |
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| 1A |
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| Alkali Metals properties |
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| Soft, shiny metals Good conductors of electricity and Heat React vigorously with water Form a white product when they react with oxygen Hydrogen is not an alkali metal |
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| Alkaline Earth Metals properties |
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| Soft Shiny Metals Conductors of Heat and Electricity Reactive, but not as much as group 1 metals |
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| Halogens properties |
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| React with most elements |
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| Noble gases |
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| gases nonreactive Only a few compounds with other elements are known |
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| Alkali Metals Group |
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| 1A or 1 |
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| Alkaline Earth Metals Group |
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| 2A or 2 |
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| Halogens Group |
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| 7A or 17 |
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| Noble Gas Group |
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| 8A or 18 |
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| Metals are located |
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| on the left, except for hydrogen |
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| Nonmetals are located |
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| to the right |
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| Metalloids are located |
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| along the heavy zigzag line between the metals and nonmetals |
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| Properties of metals |
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| Metals are shiny solids except for mercury which is a liquid) Malleable and ductile They are good conductors of heat and electricity. Melt at high temperatures Have high densities |
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| Properties of nonmetals |
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| Nonmetals are dull brittle solids or gases at room temperatures. Poor conductors They are good insulators Melt at low temperatures Have low densities |
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| Properties of Metalloids |
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| Elements that have some properties similar metals and nonmetals Are better conductors then nonmetals but not as good as metals Are used as semiconductors and insulators |
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| All elements are made up of |
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| elements |
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| All atoms of the same element are |
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| identical |
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| Atoms are |
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| the smallest particle of an element that contain the characteristics of that element |
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| Dalton's Atomic theory-John Dalton |
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| Every element is made up of tiny particles called atoms All atoms of a given element are identical. They are different from atoms of other elements. Atoms of two or more different elements combine in a definite proportion to form compounds. A chemical reaction involves changes in the arrangement or combination of atoms. (Atoms are neither created or destroyed) |
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| Electron Charge |
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| Negative |
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| Proton charge |
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| Positive Charge |
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| Protons and Neutrons are contained to |
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| A small region called the nucleus |
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| Neutrons charge |
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| neutral |
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| An atom consists |
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| of a nucleus that contains protons and neutrons |
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| Electrons are constantly moving in the large empty space around the nucleus |
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| called the electron cloud |
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| An atom of any element is electrically |
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| neutral the net charge of an atom is zero |
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| For a neutral atom |
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| protons=electrons in numbers |
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| The of which subatomic particle is negligible |
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| electron |
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| Where most of the mass in a atom |
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| the nucleus |
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| Chemist use atomic mass units |
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| to give masses of atoms and subatomic particles |
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| 1amu= |
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| 1/12 the mass of a C-12 atom with 6 protons and 6 neutrons |
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| Atomic Number is equal to the number |
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| of protons in an atom |
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| Atomic Number Appears |
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| above the the symbol of an element in the periodic table different from the nuclear symbol |
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| Mass Number |
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| is the sum of the number of protons and number of neutrons in the nucleus. |
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| Mass number= |
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| number of protons+number of neutrons |
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| Isotopes |
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| are atoms of the same element that have different mass numbers. They have the same number of protons but different number of neutrons |
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| Nuclear Symbols |
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| Helpful when specifying isotopes. Gives the Mass number in the upper left hand corner and the atomic number in the lower left corner. |
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| Atomic Mass is listed |
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| below the symbol of each element on the periodic table |
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| Atomic Mass gives the |
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| average of the atom |
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| Atom mass is |
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| a weighted average of masses of all isotopes based on their fractional natural abundances |
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| Electromagnetic Radiation |
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| Is energy that travels as waves through space Moves at the speed of light in a vacuum Is described in terms of wavelength and frequency |
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| Wavelength (lamda) |
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| is the distance between the top of a wave to the top of the next wave is expressed in meters (m) |
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| Frequency (v,nu) |
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| is the number of waves that pass by each second Is expressed in cycles per second also uses hertz |
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| Speed of light(c)= |
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| frequency x wavelength |
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| Electromagnetic Spectrum is |
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| a collection of all forms of electromagnetic radiation |
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| Visible light within |
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| wavelengths 700-400nm |
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| White light that passes through a prism |
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| is separated into all colors called a continuous spectrum. gives the colors of a rainbow |
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| Atomic Spectrum |
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| consists of lines of different colors (line spectrum) |
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| What causes an atomic spectrum |
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| formed when light from a heated element passes through a prism. |
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| When an electron jumps to a higher energy level it |
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| absorbs energy |
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| An electron falls to a lower energy level by |
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| emitting energy |
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| Emitted radiation consists of small particles called |
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| photons |
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| The formula for the maximum number of electrons a energy level can hold |
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| 2n^2 |
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| the number of sublevels in an energy level is equal to |
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| the principal quantum number (n) |
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| Sub levels are designated with the letters |
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| s p d f |
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| Sublevels are also known as |
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| subshells |
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| maximum number of electrons in s |
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| 2 |
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| maximum number of electrons in p |
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| 6 |
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| maximum number of electrons in d |
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| 10 |
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| maximum number of electrons in f |
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| 14 |
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| S orbitals |
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| has one orbital that holds 2 electrons |
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| P orbitals |
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| have 3 orbitals and can hold 6 electrons |
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| d orbitals |
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| have 5 orbitals and can hold 10 electrons |
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| f orbitals |
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| have 7 orbitals and can hold 14 electrons |
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| Valence Electrons are |
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| the electrons in the highest (outermost) energy level |
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| Valence electrons in the electron configuration are the electrons in sublevels |
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| s and p with the highest n number |
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| All elements in the same group have |
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| the same number of valence electrons |
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| Number of valence electrons equal the |
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| group number if using the the 1a-8a numbering system |
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| Number of valence electrons equal |
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| group number - 10 if you are using the 1-18 numbering system |
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| Atomic radius is |
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| the distance from the nucleus to the valence electrons |
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| Atomic radius increases going down each group of Representative elements because |
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| the number of energy levels increases |
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| Atomic radius decreases going left to right across a period as |
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| more protons increase nuclear attraction for valence electrons |
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| Ionization energy is |
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| the energy it takes to remove a valence electron |
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| Metals have 1-3 valence electrons |
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| lower ionization energy |
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| Non metals have 5-7 valence electrons |
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| higher ionization energy |
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| Nobel Gases have complete octets (He has two valence electrons) |
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| have the highest ionization energies in each period |
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