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Chemistry Flashcards

Terry Boot Science Grade 10 English 71 cards

Chemistry Flashcards

Cards in this deck (71)

  1. 1Copper's periodic table informationAtomic Number: 29
    Atomic Mass: 63.55
    Boiling point: 2562
    Melting point: 1085
    Charge(s):2+,1+
  2. 2Aggressively seeks 1 ion to complete its shellHalogens
  3. 3Has a completely stable outer shell and is very unreactiveNoble Gases
  4. 4A model of the atom that states matter is composed of atoms, atoms of the same element are identical, and compounds are combinations of atoms.Dalton's Billiard Ball Model
  5. 5A model that discovered the nucleus and stated that electrons were found in the outer region(and equal to the number of protons). It also hypothesized the existence of neutrons. Stated isotopes existed, and that atoms of the same element are chemically alike but differ in mass.Rutherford's Solar System Model
  6. 6Discovered electrons, which had a negative charge. Said that it was one giant positive charge with negative electrons embedded inside it.Thomson's "Plum Pudding" ModelDiscovered electrons, which had a negative charge. Said that it was one giant positive charge with negative electrons embedded inside it.
  7. 7Hypothesized the existence of electron shells, where they sit, and only a certain number. Shows the distribution of electrons. 2 in the first shell, 8 in the 2nd shell etc.Bohr's Orbital Model of the Atom
  8. 8Transition MetalsExhibit multi-valency. They have more than
    one charge.
  9. 9IsotopesAtoms of the same element that are chemically alike, but differ in terms of mass.
  10. 10Significance of the group number when talking about electronsStates how many valence electrons there are. Ex. Oxygen is group 16. 16-10=6. Oxygen will have 6 valence electrons.
  11. 11How does an atom become an ion?By gaining or losing electrons and taking on a charge
  12. 12What are the two types of ions and what are their differences?Cations are positive. When metals lose electrons. Anions are negative and occur when non-metals gain electrons(because electrons have a negative charge).
  13. 13Which atom is neutral?Neutron? (just think= Neu - tral. Neu - tron.)
  14. 14What type of ion would Oxygen be?Anion, because it is negative.
  15. 15What does Isoelectronic mean?It means that the ions have the same number of electrons as a noble gas. Ex. Neon has 10 protons and 10 electrons. Sodium ion(Na+) has 11 protons and 10 electrons. Sodium is isoelectronic to Neon.
  16. 16How do elements form compounds?Valence electrons interact when atoms collide to complete their outer shell so they can be stable. Metals usually lose electrons, non-metals usually gain electrons, and they can also share electrons(which forms compounds).
  17. 17What are bonds of electrons, and what are the two types?Forces that hold groups of atoms together so they function as a unit. Ionic bonds are the transfer of electrons(thus becoming negative or positive) and covalent bonds are the sharing of electrons.
  18. 18How do ionic compounds form?There is a complete transfer of electrons. Metals want to lose electrons, non-metals want to gain electrons. A ionic bond forms between the oppositely charged ions. Made of a non-metal and a metal.
  19. 19How do molecular compounds form, and what are they made of?Sharing electrons. They are made of non-metal atoms(not ions). Electrons are distributed between the atoms. Forms a covalent bond because they all want valence electrons to fill their outer shells. They obtain a valence electron configuration like the nearest noble gas.
  20. 20What is the difference between monoatomic and polyatomic?Mono=one. It means that a compound or element only has one ion. Polyatomic means a molecular compound that has a charge and becomes a polyatomic ion.
  21. 21How do you name molecular compounds? What is the difference between them and ionic naming?You take the name and add -ide at the end of the non-metal in ionic compounds. In molecular compounds, you add di, tri, tetra, etc. depending on how many of the second non-metal there are.
  22. 22Give the name of NaClSodium Chlorine = Sodium Chloride
  23. 23Give the name of SiO2Silicon Dioxide
  24. 24ICl3Iodine Trichloride
  25. 25N203Dinitrogen Trioxide
  26. 26Where are the multivalent metals on the periodic table?In the middle. They have more than one charge.
  27. 27Give the name of Iron(III) OxideFe2O3
  28. 28How does the melting point compare between ionic and molecular compounds?It is higher for ionic compounds(ex. NaF 993 C) and low for molecular compounds. Because the bonding is stronger in ionic.
  29. 29What is the difference in solubility for molecular and ionic compounds?Molecular are either soluble or insoluble, while it is slightly soluble or very soluble for ionic compounds. So if you see insoluble, it has to be molecular.
  30. 30How does the conducting differ between ionic and molecular compounds?Ionic compounds conduct electricity(because they have a metal in them), molecular compounds do not.
  31. 31What phase is molecular compounds at room temperature?It can be either solid, liquid, or gas at room temperature. As for ionic compounds, it is always solid at room temp.
  32. 32What about the hardness in molecular and ionic compounds?Ionic compounds are hard and brittle, while molecular compounds tend to be more soft or even liquid(because the chemical bonding is stronger in ionic)
  33. 33What are ionic compounds made of, and what about molecular compounds?Ionic compounds are composed of ions. Molecular compounds are composed of covalently bonded atoms.
  34. 34Give the written formula of P502Tetraphosphorus Dioxide
  35. 35Make a mnemonic for remembering the order of the models of the atom.BPSO
    Big Poe So-neutrons Old
  36. 36Which type of compound is odorous?Molecular compounds.
  37. 37How do you name bases?They always have hydroxide ion(OH) attached and so are easy to spot. They are always aqueous.
  38. 38Name NaOH and CuOHSodium Hydroxide. Copper(I) Hydroxide.
  39. 39Aluminum HydroxideAl(OH)3
  40. 40Do acids contain ions?NO! They are molecular compounds. They form ions after being dissolved in water, though.
  41. 41How can you tell something is an acid?If it has an H(Hydrogen) at the beginning of a formula or a COOH at the end. The state of an acid has to be aqueous.
  42. 42Give the acid name of Hydrogen Chloride.Hydrochloric acid. (because if it is hydrogen~ide, it becomes hydro~ic).
  43. 43Acid name of Hydrogen phosphatePhosphoric acid(because if it ends in ate, it becomes ic).
  44. 44Acid name of HNO2Nitrous acid(Ite becomes ous).
  45. 45CH3COOHHydrogen acetate>>>acetic acid
  46. 46Acids turn litmus paper ____ and bases turn litmus paper ___.Red, blue
  47. 47Acids taste ____, Bases taste ____ and feel ____.Sour, bitter, slippery.
  48. 48If the ph of a chemical is less than 7, what is it?An acid. If it was more than 7, it would be a base.
  49. 49What is the ph of pure water?7. It is neutral.
  50. 50What is the ph of sea water?Around 8 to 9 ph. So it is a base. Normal rain water is 5.5 and is an acid.
  51. 51What is the acid base neutralization?Where an acid reacts with a base and becomes a ionic compound and water. ex. HCL+NaOH = NaCl + H20. Is a type of double replacement reaction.
  52. 52If a reaction is releasing energy, is it exothermic or endothermic?Exothermic. As in exit.
  53. 53If an reaction is absorbing energy, on what side will energy be?On the left, with the reactants. It will be on the right if it is releasing energy.
  54. 54What is the law of conversation of mass?States that mass is neither created or destroyed in an ordinary chemical reaction. So the mass of the reactants must equal the mass of the productions.
  55. 55Balance the equation: _H2+_02>_H202H20+02>2H20
  56. 56Write this equation out in words. CH8(g)+5O2(g) > 3CO2(g) + 4H20(g)Propane reacts with oxygen to produce carbon dioxide gas and water vapour.
  57. 57What are the diatomic and polyatomic molecular elements?Cl2,H2, 02,N2, F2,I2, BR2, P4, S8
  58. 58What are the five types of reactions?Formation, Decomposition, Single replacement, double replacement, hydrocarbon combustion(where something reacts with 02)
  59. 59In scientific notation when moving the decimal, when will it be negative, and when will it be positive?It is negative if you are moving right and positive if you are moving left. Ex. 2234. = 2.234x10^3
  60. 60What is avogadro's number?6.02x10^23 of anything. Used to measure the number of atoms/molecules/formula units/ions in something.
  61. 61What is the unit for an mole of an ionic compound?Formula Units.
  62. 621 mole of CuSO4 has...6.02x10^23 formula units(because it is an ionic compound)
  63. 63How many grams are in 5.6 moles of Fe?312.76 grams of Fe.
  64. 64How many molecules of O are present in 78.1 g of oxygen gas?1.47x10^24 molecules of O2
  65. 65How many moles and atoms of Cu are present in 35.4 g of Cu?.5570416994 moles. 3.35x10^23 atoms.
  66. 66Calculate the mass of 6.99x10^25 molecules of Cl28.23x10^4 g Cl2
  67. 67How many molecules are in 40.0 g of water?1.34x10^24 molecules H20
  68. 68Calculate the number of moles of I2 in 3.01x10^22.0.0500 moles.
    0.05 moles.
  69. 69In a chemical reaction what is conserved and what isn't conserved?Atoms and mass(law of conversation) are conserved. Molecules and moles are not conserved.
  70. 70A hydrocarbon combustion reaction is when C,H,and O compound + 02 creates CO2 and H20. True or false?True.
  71. 71Did you like this test?Yes! :)

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Grade 10 Science Flashcards on Chemistry Flashcards, created by Terry Boot on 18/01/2017.
Created by
Terry Boot · Jan 2017
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Jan 20, 2017
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