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sodium calcium aluminum ammonium

sodium calcium aluminum ammonium. chloride oxide hydroxide phosphide phosphate. Your turn : Use the following ions to make as many compounds as you can. You may use page 169 of your text book. Cl 1- O 2- (OH) 1- P 3- PO 4 3-. Na +. Ca 2+. Al 3+. NH 4 1+. Cl 1-. NaCl. CaCl 2.

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sodium calcium aluminum ammonium

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  1. sodium calcium aluminum ammonium chloride oxide hydroxide phosphide phosphate Your turn: Use the following ions to make as many compounds as you can. You may use page 169 of your text book. • Cl1- • O2- • (OH)1- • P3- • PO43- Na+ Ca2+ Al3+ NH41+ Cl1- NaCl CaCl2 AlCl3 NH 4Cl O2- Al2O3 (NH4)2O Na 2O CaO (OH)1- NaOH Al(OH)3 NH4OH Ca(OH)2 P3- Na3P Ca3P2 AlP (NH4)3P

  2. potassium magnesium Gallium Lithium chloride oxide hydroxide phosphide phosphate Your turn: Use the following ions to make as many compounds as you can. You may use page 169 of your text book. • Cl1- • O2- • (OH)1- • P3- • PO43- K+ Mg2+ Ga3+ Li1+ Cl1- KCl MgCl2 GaCl3 LiCl O2- Ga2O3 Li2O K 2O MgO (OH)1- KOH Ga(OH)3 LiOH Mg(OH)2 P3- K3P Mg3P2 GaP Li3P

  3. Lets picture what happens • Na+ + Cl- are attracted to each other. • Na+ and O2- are attracted to each other. Cl- Na+ O2- Na+ Na+

  4. What is Chemistry? What are the branches of Chemistry. Describe: Chemistry is a physical science, where we learn about matter and its changes. Organic Inorganic Biochemistry Analytical Physical Chemistry Organic = Carbon compounds Inorganic = Other compounds Biochemistry= Biological Molecules (DNA, RNA, proteins, Cofactors or coenzymes,….) Analytical = finding unknowns (like in a drug lab for forensics) Physical Chemistry = mathematics, study of subatomic particles, study of physical properties of fluids,…. Study For Finals

  5. Physical properties describe how things look, feel, … color density size boiling point melting point etc. Physical changes describe reversible changes,… melting boiling ripping mixing ….. What are physical properties? Physical changes?

  6. Chemical properties are the expected behaviors of substances reactivity stability Can only be observed by changing the identity of the substance Chemical changes are the actual occurrence of the change oxygen reacts with iron to produce rust zinc reacts with acid to make hydrogen and a zinc salt. What are chemical properties? Chemical changes?

  7. Homogeneous means the same throughout. solutions pure substances. elements compounds ionic compounds Heterogeneous means having different phases mixtures (only) you can see particles in this, it may scatter light as in Tyndall effect (Earth Science) Homogeneous and heterogeneous?

  8. Testable – if you cannot test a theory, it is not a theory! Theories can be supported – not proven! Laws are generalizations of known facts often are expressed as mathematical expressions. Theories must be:Laws are:

  9. D = mass/volume mass = DV V = mass/D Multiply to find mass Divide to find volume or density. Always divide denominator, always multiply numerator! Density calculations use what formula? When do you multiply, when do you divide?

  10. MASS VOLUME DENSITY HEAT SPECIFIC HEAT TEMPERATURE GRAMS, g mL, cm3, dm3,L … g/L, mg/mL, kg/dm3 Joules J/goC oC or kelvin What are the units of the following quantities?

  11. #25 What is the density of a piece of cork that has a mass of 0.650g and a volume of 2.71cm3?Step 2: Plan how to solve the problem • D =? • D = mass  volume • Mass = 0.650 g • Volume = 2.71 cm3 • Substitute numbers for symbols and press buttons on your calculator.

  12. 26.Barium Perchlorate has a density of 2.74g/cm3. What is the mass? of 27.2 cm3 of this substance? M = DV Density = 2.74 g/cm3 Volume = 27.2 cm3 Mass = (2.74 g/cm3)(27.2 cm3) Mass = 74.5 g Does this make sense? What happened to the cm3?

  13. List the postulates of Dalton’s Atomic Theory. • Elements are made of tiny particles called atoms. • All atoms of a given element are identical. • All atoms of a given element are different from the atoms of other elements. • Atoms can combine with each other(in small whole number ratios) to form different compounds. (ex: NO, NO2, N2O) • Atoms are indivisible.

  14. Whose experiment found the charge to mass ratio of electrons? • Millikan

  15. What discovery led to the change from all atoms of the same element are identical, to all atoms of the same element are chemically identical? • The discovery of isotopes.

  16. What are isotopes? • Atoms of the same element with different numbers of neutrons. • They have different masses, but the same chemical properties.

  17. If an element has 15 protons, list its atomic number and symbol • Atomic number 15, P If an element has a mass of 32, and 15 protons, name the isotope. • P- 32 also written as 32P 15 How many electrons does this substance have? How many neutrons? • P has 15 electrons and 32-15 = 17 neutrons.

  18. Which law does this illustrate? Who discovered it? The Law of Conservation of Matter, discovered by Lavoisier.

  19. Which law does this illustrate? Whois credited with this Law. The Law of Multiple proportions. Dalton.

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