Atomic mass units (amu) help us mathematically \'deal\' with the smallness of th
ID: 913305 • Letter: A
Question
Atomic mass units (amu) help us mathematically 'deal' with the smallness of the mass at the atomic level. 1 amu = 1.66 x 10^-24 grams ......wow that is small!! By definition one 12^C atom has the mass of 12 amu. Find this information in your Periodic Table, why is the value in the Periodic Table slightly larger than 12 There are three types of elements on the Periodic Table. What are they ________________, ________________, _____________ And where can they be found on the Periodic Table Some groups of the periodic table are lucky enough to have their own names, which groups are those and what are their names (Use the textbook, not Wikipedia) What is the difference between a molecular formula and an empirical formula A cation is:__________ An anion is:_______ Look at the group 7A, 6A and 5A anions on the period table and their charge. Give logical reason for their charge As we look at nomenclature of compounds there will be a distinct set of rules for naming ionic compounds (salts) versus molecular compounds. Ionic compounds are composed of cations (metals with a + charge) and anions (non-metals with a - charge) and molecular compounds are composed of only non-metals. Which type of compound (ionic or molecular) is each of the following sodium chloride _________ MgSO_4_________ dinitrogen tetroxide _________ P_4 S_10 _______Explanation / Answer
3.
The atomic mass given in the periodic table is a “weighted” average of all three isotopes of carbon found in nature.
It means that if one particular isotope occurs much more than the others, then the weight of that isotope should have more impact on the overall average.
The percent abundance of carbon-12 is around 99%, where as Carbon-13 and Carbon-14 both occur less than 1% each in nature.
Hence the AMU of the Carbon-12 (12 amu) would have the greatest impact.
However, the C-13 and C-14 exist in very small quantities which is the reason Carbon in general has an atomic mass of slightly higher than 12, 12.011, to account for the small changes incurred by C-13 and C-14 atoms.
4.
a. Three types of elements: metals, nonmetals, and metalloids.
b. Following are the lucky groups that got their own names on periodic table-
1A – Alkali Metals
2A – Alkaline Metals
7A – Halogens
8A – Noble gases.
5.
The empirical formula has the smallest whole number for their subscript whereas the molecular formula is the actual number of molecules or atoms in a compound.
The empirical formula is the simplest form of the molecular formula. For example;
Molecular formula - C6H12
Empirical formula - Divide by 6 - CH2
6.
a. In simple words-
Cations: +
Anions: -
Ions: all cations and anions
b. In group 5A, we have 5 - 8 = -3, so we expect N3- for nitrogen and P3- for phosphorous. This pattern is broken with bismuth at the bottom of the column because it is a metal. Remember that metals form positive ions. Bismuth forms Bi3+ ions.
In group 6A we have 6 - 8 = -2, so we expect O2- for oxygen and S2- for sulfur, the two elements we usually deal with in this column.
In group 7A we have 7 - 8 = -1 so we expect F-, Cl-, Br-, and I-. We will not deal with astitine (At)
7.
a. NaCl- Ionic
b. MgSO4- Ionic
c. Dinitrogen tetroxide- Molecular
d. P4S10- Molecular.
Hope this will help you. For any question regarding my answer, write me in comment.
If satisfied with answer, please leave positive feedback. Thanks.
Answer of your question that yiu asked in comment-
a.
One of the postulates that is not considered true today is that atoms are indivisible.He said that all atoms of a given element are alike. This is not true due to the existence of isotopes. Isotopes are atoms of the same element that have different masses because they have different numbers of neutrons. During a chemical reaction, atoms can change their identities.
b.
The law of constant composition says that any given compound always consists of the same atoms and the same ratio of atoms.
The law of conservation of mass says that the total mass of materials before and after a chemical reaction must be the same.
2.
a. Atom consists of three subatomic particles: protons, neutrons, and electrons .
The nucleus contains only Protons and neutrons are called nucleons.
b.
Mass of Proton- 1.67262 X 10^-27
Mass of Electron 0.00091 X 10^-27
Mass of Proton/Mass of Electron
1.67262 X 10^-27/ 0.00091 X 10^-27= 1838.04 g
So therefore it would take 1838.04g of electrons to equal the mass of a proton.
c.
Atomic mass: 12.0107 u ± 0.0008 u
Atomic number: 6
Yes it is different, this is due to other isotopes that I already explained in last question.
d.
Neutrons.
Ok …good luck..
Just confirm me once you got this answer....
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.