Groups vs. Periods what s the difference?? Groups: Periods:
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- Clarence Henry
- 5 years ago
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1 Before watching the video: Use page 131 in your book or the internet to label the periodic table according to the following guidelines (NOTE: Your key might not look exactly like the book!!!) a. Color all metals blue b. Color all non-metals yellow c. Draw a dark line showing the transition between metals and non-metals (the line by the semi-metals) d. Identify the transition metals e. Label the halogens f. Label the alkali metals g. Label the alkaline earth metals h. Label the noble gases i. Number all groups and periods on the periodic table Groups vs. Periods what s the difference?? Groups: 1. Identify which two elements are most similar chemically: a. Mg Cs Zr Al Ca b. Cl Nb S Br Kr Periods: 2. Are the metals on the left or right side of the periodic table? 3. What are the group numbers for the transition metals?
2 Group 1 Group 2 Groups 3-12 Group 17 Group 18 Name Metal or nonmetal? State at 25 o C and 1 atm Malleable and ductile (Y or N) Conducts electricity (Y or N) Key physical properties. Key chemical properties Define these terms: 1. Malleable 2. Ductile 3. Luster 1. What types of elements are malleable and ductile? 2. What phase (solid/liquid/gas) are the majority of the elements in? 3. Which group has elements that exist in all the phases? 4. What is special about the noble gases? 5. What type of elements conduct electricity?
3 Atomic Radius (atomic radii): Electronegativity: Ionization Energy: Ionic Radius (Ionic Radii): 1. Which atom/element is larger? Rb or Pb 2. What is the largest element? 3. What is the most electronegative element? 4. How is ionic radius different from atomic radius? 5. Which element has a higher ionization energy? K or Ga 6. Which element has a higher ionization energy? Li or Rb 7. How are electronegativity and ionization energy are related? What is the pattern between these two trends?
4 Define atom: John Dalton: (1) Proposed: all elements are composed of very small particles called atoms which are indivisible. (2) Proposed: All atoms of the same elements are identical. (3) Proposed: Atoms of different elements are different. (4) Proposed: Atoms of different elements can combine with each other only in simple whole number ratios to form compounds. Electron Stream w/o applied electric field Stream after applying field, + on top, - on bottom Electron (5) Proposed: Chemical reactions occur when atoms are separated, joined or arranged. However, atoms of one element ARE NOT changed into atoms of another element by a chemical reaction. (Only by nuclear reactions) JJ Thomson: What did he discover? With what experiment? What was his proposition and was it true? + Magnetic field - Magnetic field Electron Stream w/o applied electric field Electron Stream after applying field, + on top, - on bottom How did the cathode ray tube experiment prove that electrons exist and they are negative?
5 JJ Thomson (second proposition): What was Thomson s second proposition? What is true? Why or why not?? Ernest Rutherford: What was his proposition? What is true? What were the results of the gold foil experiment? Why were some of the particles deflected? Niels Bohr: Proposed Proposed -
6 Components of the Atom: Protons: Neutrons: Electrons: Atoms are always, meaning they have the same number of. Atomic Number: Mass Number: Atomic Mass: Isotopes: What are isotopes and how are they different? 1. What s the difference between mass number and atomic mass? 2. How is the mass number calculated? 3. Where can the atomic mass be found? 4. How many protons are in sodium and how do you know? 5. How many electrons does a calcium atom have? How do you know? 6. What happens if the atomic number changes? Example: Identify how many protons and neutrons are in the following group of isotopes Hyphen Notation is Name Mass # Carbon-12 Carbon-13 Carbon-14 Calculating Atomic Mass: Example: Naturally occurring chlorine is 75.53% chlorine-35 and 24.47% chlorine-37. What is the average atomic mass which should be placed on the Periodic Table for the element? Example: The element neon consists of three isotopes with masses of 19.99, and amu. These three isotopes are present in nature to the extent of 90.92%, 0.25% and 8.83% respectively. Calculate the atomic weight of neon. 7. How many neutrons are in Uranium 235? 8. What is the identity of an element with 3 protons, 4 neutrons and 3 electrons? 9. Write the hyphen notation for the element in #8. Calculate the average atomic mass of lithium, which occurs as two isotopes that have the following atomic masses and abundances in nature: amu at 7.30% and amu at 92.70%.
7 Ions: What are they and how are they different? 1. The sulfide ion has a charge of 2. How many protons and electrons does this ion have? IF: #electrons < #protons (electrons are given or lost) then there is an excess charge and it s called a IF: #electrons > #protons (electrons are gained) then there is an excess charge and it s called an 2. An element has 20 protons and 18 electrons. Identify the element and determine the ionic charge. 3. A magnesium ion has a +2 charge and a mass number of 25. How many protons, neutrons and electrons are there? Chemical Configuration/Nuclear Symbol: mass number atomic number 16 O 2-8 ionic charge Protons Electrons Neutrons Mass # Atomic # Charge NUCLEAR SYMBOL B 14 6 C S Al Cr
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