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Name: _________________________________ 3. Each row in the periodic table is called a ________________ Periodic Table Trends 4. Elements in the same period share the same Organization of the Periodic Table 1. First created by Dmitri Mendeleev A. Organized atoms by ________________________ __________________________. Noble Gases B. This was ok, but trends in the periodic table did not match up C. Mendeleev was able to predict how elements interacted with each other and wanted his table to display those trends. Henry Moseley 1. Took the ____________________charge, which is the number of protons in the nucleus, and ordered the periodic table using the number of protons in the atom. 2. The trends found by Mendeleev were in place. Periodic Law 1. States that physical and chemical properties of elements are properties of their ___________________________________. 2. Each column on the periodic table is called a ______________ A. Groups have the same number of _____________________________ in their outer-most sublevel 1. Group _______ 2. Have filled ____ and ____ orbitals 3. Are very _________________. Do not form bonds with other molecules 4. All atoms desire to be noble gases and will ____________ or __________electrons from other atoms to do so. A. This is how a _________________________________ is made 5. To act like noble gases, atoms will take the easiest route, and either give up electrons or gain them Alkaline Earth Metals Alkali Metals 1. Group _____ 1. Found in ________________________ 2. Made of _________________________ (meaning easy to bend) 3. Outer electron shell has an _______ configuration 4. React quickly with ______________ or ________ A. Can create a basic _________________ with water 5. Have an extra electron to give up in order to form a _______ ion. 2. Outershell has a ________configuration 3. Metals are ]____________ and __________ reactive 4. Become ions with a _____ charge Transition Metals 3. Some glow when electrons hit them. 4. _______ series Actinides 1. Groups __________________ 2. __________________ metals and even ___________ reactive than groups 1 and 2 Lanthanides 1. ____ series 2. All are ________________ A. ___________________ important for nuclear reactions B. Many are man-made Main Block Elements 1. Groups 3A-8A 2. Made of ______________________________________________________ 1. Contain atomic numbers 57-71 2. Shiny and reactive _______________ _____________________ A. Metal examples: aluminum, gallium, indium, tin thallium, lead, bismuth, polonium B. Metalloids: boron, silicon, germanium, arsenic, antimony, and tellurium. C. Nonmetal examples: hydrogen, oxygen, nitrogen, carbon, phosphorus, sulfur, selenium, fluoride, chlorine, bromide, iodine, and noble gases configuration A. Become a ________ ion if this happens Chalcogens 3. The periodic _________________________: The area on the periodic table that divides the metals from the nonmetals 1. Group _____ A. Atoms around the stair step are ___________________ i. Metalloids have characteristics of nonmetals and metals ii. Metalloids are also termed 2. Try to gain two electrons to have a noble gas electron configuration. A. Become a _____ ion if this happens Periodic Trends ________________________________ 1. The four different trends to know include: Halogens A. ________________________________________ B. ________________________________________ C. ________________________________________ D. E. ________________________________________ Electronegativity 1. Defined by an atoms tendency to attract electrons in a chemical bond. 1. Group _____ 2. In a chemical bond, atoms have to 2. Form salts with __________________ metals _____________________________________ 3. The most ____________________ nonmetals 4. ______________________ electrons to have a noble gas 3. The atom with a higher electronegativity will keep the electrons closer to it. 4. Atoms with the highest electronegativity are found in the _____________________________ an atom contains. ____________________-side of the periodic table; excluding 1. This means, assuming the atom looks like a sphere, the noble gases. ______________________ of the atom would increase as you go down the 5. The atom with the highest electronegativity is periodic table. ______________________ 3. The top, right-area of the periodic table has the smallest atomic 1. The lowest is ___________________ radius ____________________ Atomic Radius 4. Which would you assume to have the largest atomic radius: Al, Al+, or Al5. Which would you assume to have the smallest atomic radius: C2+, C+, C, C-, C21. Atoms with the largest atomic radius are found at _______________________________-side of the periodic table 2. The further you go down the periodic table, the more PROBLEM: Using only the periodic table, rank each set of main group elements in order of decreasing atomic size: (a) Ca, Mg, Sr (b) K, Ga, Ca (c) Br, Rb, Kr (d) Sr, Ca, Rb Electron Affinity 1. The ability of an atom to ___________________ and hold onto an atom. Ionization Energy 1. Defined as the energy needed to remove an electron from an atom 2. The __________________________-area of the periodic table contains the atoms with the highest ionization energy. 2. Electron affinity is highest in the ________________________________________ of the periodic table. 3. _________________ has the highest ionization energy 3. _______________ has the highest electron affinity. PROBLEM: Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE1: (a) Kr, He, Ar (b) Sb, Te, Sn (c) K, Ca, Rb (d) I, Xe, Cs 4. _____________________________: inner electrons are shielded by outer electrons, so outer electrons are removed before inner electrons. A. That is why _____________________ is so reactive. It quickly reacts with something around it. B. Electrons in the outer energy levels feel _______ of the nuclear charge (they feel ________ of the positive charge). C. This is commonly referred to as ________________________________. Most trends can be described by the shielding effect and effective nuclear charge.