3.2. Give the symbol including mass number the following: 3.2.1. The ion with 22 protons, 26 neutrons and 19 electrons 3.2.2. The ion of Sulphur that has 16 neutrons and 18 electrons-
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- Give the symbol for an element that is : 1. A transition metal in the fourth period from the following list :Ti, Ne, Ce, W. ( ). 2. A metalloid =3. A non- metal in group 4A, 5A, or 6A=4. A lanthanide =5. A metal in group 3A or 4Abottle. The bottle contains 3.78 L of ethanol. The bottle contains 2.948 x 105 cg of ethanol. volumes the same? 22,23) Ethanol (also known as ethyl alcohol) arrives from the chemical supplier in a plastic What is the density of ethanol in g/mL? 24,25) A naturally occurring sample of magnesium has three isotopes with the following percent abundances and isotope masses: 24Mg 25Mg 26M9 78.99 % 23.98504170 amu 24.98583692 amu 25.98259293 amu 10.00 % 11.01 % What is the atomic mass of magnesium based on this information?(2.8)An element occurs as three isotopes with atomic masses 19.99 amu (abundance = 90.51%), 20.99 amu (abundance = 0.27%), and 21.99 amu (abundance 9.22%). What is the atomic mass of the element? 62.97 amu 20.18 amu 21.00 amu 21.01 amu
- Titanium has five common isotopes: 46Ti (8.000%, 45.95 amu), 47 T (7.800%, 46.95 amu), 48Ti (73.40%, 47.95 amu), 49Ti (5.500%, 48.95 amu) 50 Ti (5.300\% , 49.95 amu). What is the average atomic mass of titanium ? (2 decimal places)49.31%. What is the relative atomic mass of Br? 2.9. An isotope of lead has an isotopic mass of 208. Give the appropriate notation for the isotope. 2.10. Thallium has two naturally occurring isotopes, 203TI and 205TI and has an average atomic mass of 204.39 u. Tl-205 has an abundance of 70.48%. What is the percent natural abundance of Tl-203? 2.11. What is the oxidation number of Xe in Xe0,4? 212 What is the ovidation pumber of S in SaO.Ch?3.1. Consider ¹2C, 13C and 13C- How many neutrons are found on each? How many electrons are found on each?
- II. COMPLETING THE TABLE. Fill in the gaps in the following table. Follow the number sequence indicated in the parenthesis,( ), to answer the missing data. (10 points) Number of neutrons Number of electrons (3) 88 (8) (10) Number of Atomic number 30 Mass number (1) 226 Atom protons (2) (5) (7) 35 35 Zn Ra Fes (4) 26 (6) (9) 45 56 Br 35 80The relative ratio, or percent, of each isotope found in nature is the abundance number used to calculate the average mass. Here's the general equation for average atomic mass: (Abundance A)(Mass A) + (Abundance B)(Mass B) = Atomic Mass For example, here's how the average mass of of boron was calculated. Percent Boron-10 Percent Boron-11 10 + 11 =10.81 amu 100 100 (.20)10 + (.80)11 = 10.8 amu %D 3. Let's try out the atomic mass equation. Suppose you have a mixture of two nitrogen isotopes. For every 1 Nitrogen-15 isotopes, there are 3 Nitrogen-14 isotopes. Determine the abundance of each isotope in this mixture. Predict the average atomic mass of this mixture. Hint: This is NOT the mixture of nitrogen found in nature. You can check your answer by clicking "My Mixture" under isotope mixture. Next, create the mixture described in the problem. 14.50 amu 14.00 amu 14.25 amu 14.75 amuUnit 4 Study Guide: Atomic Structure Atomic Theory: Be able to describe and recognize each scientists' contribution to the atomic structure. Matching format. Plum pudding model discovered electrons discovered nucleus developed planetary model of orbit developed most modern atomic model "quantum model" where electrons move around in electron clouds Who completed the gold foil experiment? Describe the general experiment and its importance. • Counting Subatomic Particles: a. List the three fundamental subatomic particles and their charge. 1. 2. 3. b. Isotopes are atoms of the same element that have different number of C. Which two subatomic particles make up the nucleus? d. Where is majority of an atom's mass concentrated? e. Which one of the subatomic particles can identify an atom? f. For the isotope Rubidium-89, list the follow characteristics of the atom. Mass # Atomic # Protons Neutrons Electrons Average atomic mass: weighted average of the mass of isotopes in a naturally occurring…
- On the planet Kracalac, in another solar system, argon has three naturally occurring isotopes as follows: Isotope Mass (amu) Natural Abundance (%) Argon-36 35.968 10.65 Argon-38 37.963 15.15 Argon-40 39.962 74.20 What is the average atomic mass of argon on Kracalac?10. Copper has two naturally occurring isotopes, 6Cu (isotopic mass = 62.9296 amu) and 6Cu (isotopic mass = 64.9278 amu). If copper has an atomic mass of 63.546 amu, what is the % abundance of each isotope?a. An element (X) is found in the (4th row & 6th group) of the periodic table. Write the symbol of this element and Classify it as: (a) metal (b) metalloid (c) non-metal b. The element (X) has 6 isotopes, one of them is 80X. Find the number of neutrons in this isotope? c. The element (X) can form two oxyanions: XO4² and XO3² , write the name of the compound Na2XO3 d. What is the mass percent of the element X in the NazXO3 compound e. What is the number of Na atoms in 0.46 moles of NazXO3? f. One important compound of X is XS2 prepared by the following equation: XO2+ Na2S → XS2 + Na2O Considering the following figure, Which compound is the limiting reactant? 1 mol of XO2 1 mol of NażS