[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-seo-572001-105":53,"doc-detail-572001-en":127},{"code":4,"msg":5,"data":6},0,"success",[7,14,19,24,29,34,39,44,49],{"id":8,"doc_module":9,"doc_module_name":10,"category_name":11,"show_sort_weight":12,"slug":13},11,1,"Template","Presentations",90,"presentations",{"id":15,"doc_module":9,"doc_module_name":10,"category_name":16,"show_sort_weight":17,"slug":18},12,"Resumes",80,"resumes",{"id":20,"doc_module":9,"doc_module_name":10,"category_name":21,"show_sort_weight":22,"slug":23},14,"Invoices",70,"invoices",{"id":25,"doc_module":9,"doc_module_name":10,"category_name":26,"show_sort_weight":27,"slug":28},15,"Posters",60,"posters",{"id":30,"doc_module":9,"doc_module_name":10,"category_name":31,"show_sort_weight":32,"slug":33},16,"Social Media",50,"social-media",{"id":35,"doc_module":9,"doc_module_name":10,"category_name":36,"show_sort_weight":37,"slug":38},17,"Forms",40,"forms",{"id":40,"doc_module":9,"doc_module_name":10,"category_name":41,"show_sort_weight":42,"slug":43},18,"Letters",30,"letters",{"id":45,"doc_module":9,"doc_module_name":10,"category_name":46,"show_sort_weight":47,"slug":48},21,"Paper Templates",5,"papers-templates",{"id":50,"doc_module":9,"doc_module_name":10,"category_name":51,"show_sort_weight":4,"slug":52},158,"General","general-158",{"code":4,"msg":54,"data":55},"ok",{"site_id":56,"language":57,"slug":58,"title":59,"keywords":60,"description":61,"schema_data":62,"social_meta":120,"head_meta":122,"extra_data":124,"updated_unix":126},105,"en","200-ways-to-pass-the-chemistry-physical-setting-regents-exam-chemistry-study-tips","200 Ways to Pass the Chemistry Physical Setting Regents Exam - Chemistry study tips","","200 Ways to Pass the Chemistry Physical Setting Regents Exam compiles a rapid list of chemistry fundamentals and exam-focused reminders. It covers atomic structure (protons, neutrons, electrons, isotopes), ions (cations/anions), key historical models, STP conditions, electron transitions and spectra, mixtures and solutions, electron configuration and orbital notation, significant-figure counting rules, molar-conversion guidance, and ion/polyatomic naming conventions. 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Protons are positively charged (+) .  \n2. Neutrons have no charge.  \n3. Electrons are small and are negatively charged (-) .  \n4. Protons & neutrons are in an atom’s nucleus (nucleons) .  \n5. Electrons are found in “clouds”(orbitals) around an atom’s nucleus.  \n6. The mass number is equal to an atom’s number of protons and neutrons added together.  \n7. The atomic number is equal to the number of protons in the nucleus of an atom.  \n8. The number of neutrons = mass number – atomic number.  \n9. Isotopes are atoms with equal numbers of protons, but differ in their neutron numbers.  \n10. Cations are positive (+) ions and form when a neutral atom loses electrons. They are smaller than their parent atom.  \n11. Anions are negative ions and form when a neutral atom gains electrons. They are larger than their parent atom.  \n12. Ernest Rutherford’s gold foil experiment showed that an atom is mostly empty space with a small, dense, positively-charged nucleus.  \n13. J.J. Thompson discovered the electron and developed the “plum-pudding” model of the atom.  \n+ - + - Positive & negative  \n+ - + - + particles spread throughout  \n- + - + entire atom.  \n -    \n14. Dalton’s model of t~~he atom was a solid sphere ~~of matter that was uniform throughout.   \n15. The Bohr Model o~~f the atom  ~~p~~la~~c~~ed ~~e~~l~~e~~ctrons in~~“planet-like” orbits around the nucleus of an atom.   \n16. The current, wave-mechanical model of the atom has electrons in “clouds”(orbitals) around the nucleus.  \n17. USE THE REFERENCE TABLES!!!  \n18. “STP”means“Standard Temperature and Pressure.” (273 Kelvin & 1 atm)  \n19. Electrons emit energy as light when they jump from higher energy levels back down to lower (ground state) energy levels. Bright line spectra are produced.  \n20. Elements are pure substances composed of only one kind of atom.  \n21. Binary compounds are substances made up of only two kinds of atoms.  \n(examples: H2O, NH3 , CO2)  \n22. Diatomic molecules are elements that form two atom molecules in their natural form at STP. Remember the phrase – “BrINClHOF” (Br2 , I2 , N2 , CL2 , H2 , O2 , F2)  \n23. Use this diagram to help determine the number of significant figures in a measured value…  \nPacific Atlantic  \nIf the decimal point is present, start counting digits from the Pacific (left) side, starting with the first non-zero digit.  \n1 2 3  \n0.00310 (3 sig. figs. ) If the decimal point is absent, start counting digits from the Atlantic (right) side, starting with the first non-zero digit.  \n3 2 1  \n31,400 (3 sig. figs. )  \n24. Solutions are the best examples of homogeneous mixtures. (Air, salt water, etc. )  \n25. Heterogeneous mixtures have discernable components and are not uniform throughout. (Chocolate-chip cookies, vegetable soup, soil, muddy water, etc. )  \n26. A solute is the substance being dissolved, while the solvent is the substance that dissolves the solute. (Water is the solvent in Kool-Aid, while sugar is the solute. )  \n27. Isotopes are written in a number of ways: C-14 is also Carbon-14, and is also mass number 14 C  \n6  \natomic number  \n28. The distribution of electrons in an atom is its electron configuration.  \n29. Electron configurations are written in the bottom center of an element’s box on the periodic table in your reference tables.  \nMg  \n12 2-8-2  \n \\# of electrons in 3rd principal energy level  \n\\# of electrons in 2nd principal energy level  \n\\# of electrons in 1st principal energy level  \n30. Use the mole triangle diagram on the next page to help you solve conversions between moles, grams, numbers of molecules/atoms, and liters of gases at STP    \nThe ~~Mole~~ ~~  Trian~~gle  \nRemember This     \nDivide In Multiply Out“DIMO”  \nYou can only move by following the arrows through the center.  \n22.4  \nMolar Mass  \nDivide & Multiply by the values next to the arrows as you go from one type of value to another.  \nMoles  \n6.02 x 1023  \nNo. of Particles  \nWay!  \nGrams  \nVolume ","cbCaioqFERc6KaLH","https://ap.wps.com/l/cbCaioqFERc6KaLH","pdf",709475,"English","# Atomic structure and models\n## Charges, nucleus, and isotopes\n# Ions and electron energy\n## Cations, anions, spectra\n# Matter classification\n## Elements, compounds, molecules\n## Mixtures and solutions\n# Measurement and calculations\n## STP and significant figures\n## Electron configurations and orbital notation\n## Mole conversions and molar mass\n# Chemical reactions and naming\n## Chemical equations and balancing\n## Reaction types\n## Naming ionic and polyatomic compounds","[{\"question\":\"How do you calculate neutrons, mass number, and atomic number?\",\"answer\":\"Use mass number = protons + neutrons, atomic number = number of protons, and neutrons = mass number - atomic number.\"},{\"question\":\"What is STP and what values does it use?\",\"answer\":\"STP means Standard Temperature and Pressure, given as 273 Kelvin and 1 atm.\"},{\"question\":\"What do the coefficients in chemical equations represent?\",\"answer\":\"Coefficients are written in front of formulas for reactants and products and provide the ratios needed to balance the equation; only coefficients can be changed when balancing.\"}]","200 Ways to Pass the Chemistry Physical Setting Regents Exam - Chemistry study tips | PDF",1791924922]