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Lecture

The particle that has the smallest mass is.docx

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Department
Biology
Course Code
BIOL 1500
Professor
George Georgopoulos

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he particle that has the smallest mass is? Select one: a. Atom b. Neutron c. Electron d. Proton Question 2 Not yet answered Marked out of 1.0 Flag question Question text Which particle always has a negative charge? Select one: a. Neutron b. Atom c. Proton d. Electron Question 3 Not yet answered Marked out of 1.0 Flag question Question text Which of the following elements requires the least amount of energy to remove an electron to form an ion? Select one: a. Ca b. K c. Na d. Mg e. Fr Question 4 Not yet answered Marked out of 1.0 Flag question Question text According to the Lewis model of the atom, the number of bonding electrons in a nitrogen atom is? Select one: a. 1 b. 2 c. 5 d. 3 e. 7 Question 5 Not yet answered Marked out of 1.0 Flag question Question text The mass number refers to Select one: a. The number of protons in the nucleus of an atom b. The total number of protons and electrons in the nucleus of an atom c. The number of neutrons in atom d. The number of electrons in an atom e. The total number of protons and neutrons of an atom Question 6 Not yet answered Marked out of 1.0 Flag question Question text Atoms of the same element which have the same number of protons but a different number of neutrons are known as Select one: a. Neutral atoms b. Molecule c. A chemical family d. Ions e. Isotopes Question 7 Not yet answered Marked out of 1.0 Flag question Question text 24 2+ 12Mg contains (note, 24 should be directly over top of the 12) Select one: a. 12 protons, 12 neutrons and 14 electrons b. 12 protons, 12 neutrons and 10 electrons c. 12 protons, 12 neutrons and 12 electrons d. 12 protons, 10 neutrons and 10 electrons e. 24 protons, 12 neutrons and 2 electrons Question 8 Not yet answered Marked out of 1.0 Flag question Question text In which pair of elements is the element with the smaller electron affinity listed first? Select one: a. Helium, neon b. Sodium, magnesium c. Fluorine, oxygen d. Beryllium, lithium Question 9 Not yet answered Marked out of 1.0 Flag question Question text Which of the following statements about atomic structure is TRUE? Select one: a. The number of protons, neutrons and electrons are always equal in a neutral atom. b. The number of neutrons and electrons are always equal in a neutral atom. c. The number of protons and neutrons are always equal in a neutral atom. d. The number of protons and electrons are always equal in a neutral atom. Question 10 Not yet answered Marked out of 1.0 Flag question Question text Which of the following is the most important factor in determining the chemical properties of an element? Select one: a. The number of valence electrons b. The total number of neutrons c. The total number of electrons in its atoms d. The total number of protons in the nucleus Question 11 Not yet answered Marked out of 1.0 Flag question Question text How many molecules are in 1 mole of Na O? 2 Select one: a. 1 b. 2 c. 3 d. 1.8x10^24 e. 6.02x10^23 Question 12 Not yet answered Marked out of 1.0 Flag question Question text 1mL is equal to how many grams? Select one: a. 2 b. 5 c. 1 d. 3 e. 4 Question 13 Not yet answered Marked out of 1.0 Flag question Question text 3mg is equivalent to how many micrograms (µg)? Select one: a. 0.000003 b. 0.0003 c. 3000 d. 0.003 e. 300 Question 14 Not yet answered Marked out of 1.0 Flag question Question text What is the difference between an ionic and covalent bond in terms of electrons. Select one: a. Ionic electrons are only lost, covalent electrons are only gained b. Ionic electrons are shared, covalent electrons are transferred c. Ionic electrons are transferred, covalent electrons are shared d. Ionic electrons are only gained, covalent electrons are only lost Question 15 Not yet answered Marked out of 1.0 Flag question Question text Determine the following for COCl 2 ·The type of bond(s) (ionic, polar covalent, non-polar covalent) present. ·If polar covalent indicate the ∆EN associated with each bond. · If polar covalent indicate the correct partial charge associated with each element of each bond.Use Lewis structure to demonstrate the electron configuration and partial charge distribution. ·Determine the potential molecular geometry. (remember VSEPR). Select one: a. Non-Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0) and double covalent to the oxygen (∆EN = 0). Molecular geometry linear. b. Polar covalent. Carbon central with double covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial negative charge, both chloride and oxygen a negative partial charge. Molecular geometry bent. c. Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial positive charge, both chloride and oxygen a negative partial charge. Molecular geometry trigonal planar. d. Ionic bond. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial positive charge, both chloride and oxygen a negative partial charge. Molecular geometry tetrahedral. e. Non -Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.89) and double covalent to the oxygen (∆EN = 0.61). Carbon partial negative charge, both chloride and oxygen a positive partial charge. Molecular geometry trigonal bipyramidal. Question16 Not yet answered Marked out of 1.0 Flag question Question text Write the equation and predict the products of the following combination.Remember to balance if necessary. Potassium iodide plus bromine gas Select one: a. KI + Br -> KBr + I b. 2KI2 + 2B3 -> K2I + 3B2 c. 2KI + Br2 -> 2KBr + I2 d. K2I3 + 4Br -> 2KBr2 + 3I Question17 Not yet answered Marked out of 1.0 Flag question Question text Balance the following chemical equations and identity the type of reaction demonstrated. Mg(NO ) +3 2PO ->3Mg 4PO ) + 3NO 4 2 3 Select one: a. Mg(NO3)2 + 3K3PO4 -> Mg3(PO4)2 + 9KNO3; combustion b. 6Mg(NO3)2 + 4K3PO4 -> 2Mg3(PO4)2 + 4KNO3; synthesis c. 3Mg(NO3)2 + 2K3PO4 -> Mg3(PO4)2 + 6KNO3; double displacement d. 12Mg(NO3)2 + K3PO4 -> 4Mg3(PO4)2 + 3KNO3; single displacement e. 2Mg(NO3)2 + K3PO4 -> Mg3(PO4)2 + 3KNO3; decomposition Question18 Not yet answered Marked out of 1.0 Flag question Question text If situated close enough together a hydrogen bond may form between which of the following. A hydrogen bond is an example of what type of attraction? Select one: a. Nδ- and Hδ-, dipole-dipole b. Oδ+ and Hδ+, ion-dipole c. Oδ- and Hδ+, ion-dipole d. Nδ- and Hδ+, dipole-dipole Question19 Not yet answered Marked out of 1.0 Flag question Question text Electrons found in which of the following orbitals have the highest energy? Select one: a. 2p b. 4p c. 3d d. 1s e. 3s Question20 Not yet answered Marked out of 1.0 Flag question Question text What volume of 0.27mol/L solution can be made using 15.2g of sodium hydroxide? Select one: a. 4.5L b. 0.27L c. 1.4L d. 15.2L e. 2.3L Question21 Not yet answered Marked out of 1.0 Flag question Question text 400mL of 3M NaOH needs to be diluted to 2M. What volume of diluting solution should be added to the initial volume? Select one: a. 400mL b. 800mL c. 600mL d. 200mL e. 100mL Question22 Not yet answered Marked out of 1.0 Flag question Question text Maganese(III) fluoride can be formed by the reaction of manganese(II) iodide with fluorine gas. If 1.23g of manganese(II) iodide reacts with 25g of fluorine gas what mass of manganese(III)fluoride is expected? Which reactant is in excess and how much of it remains at the end of the reaction? Select one: a. 0.38g, fluoride gas, 25g b. 1.23g, manganese(III) fluoride, 1g c. 0.5g, manganese(III) fluoride, 0.5g d. 0.45g, fluoride gas, 24g Question23 Not yet answered Marked out of 1.0 Flag question Question text 37.82mL of sodium hydroxide solution is needed to neutralize 15mL of 0.250mol/L of hydrofluoric acid. What is the concentration of sodium hydroxide? Select one: a. 0.0992mol/L b. 9.92mol/L c. 2.3mol/L d. 0.045mol/L e. 0.0333mol/L Question24 Not yet answered Marked out of 1.0 Flag question Question text An unknown gas is composed of 80% carbon and 20% hydrogen. A 4.60g sample occupies a volume of 2.50L at 1.50atm and 25.0 C. What is the molecular formula of the gas? Select one: a. C4H10 b. CH2 c. C2H6 d. C3H8 e. CH Question 25 Not yet answered Marked out of 1.0 Flag question Question text The name 3-ethyl-2,2-dimethyl-3-heptene tells you what about its structure. (Draw) Select one: a. 6 carbon root with a double bond at the 3rd carbon, three ethyl side chains and 2 methyl side chains. b. 6 carbon root with 3 double bonds, three ethyl side chains and four methyl side chains c. 7 carbon root with a triple bond at the 2nd carb
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