The correct answer its True
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Answer:
The correct answer is “Iron(II) sulfide.”
Explanation:
It is pretty obvious there is presented an iconic compound made by iron written as Fe and a sulfur, S that is a nonmental instead. A metal as iron will form a cation and a nonmetal an anion. The sulfur will need 2 electrons from iron in order to complete its octet and in this way the iron equilibrates the sulfur. It can give it 2, so that is why we write it in Roman numbers, and form the formula above.
By utilizing stoichiometry, we can determine that the given volume and molarity of acetic acid (HC2H3O2) would produce approximately 3.65 grams of carbon dioxide (CO2). The calculation involves determining the moles of HC2H3O2 used, which equals the moles of CO2 produced, and converting that to grams using the molar mass of CO2.
The amount of carbon dioxide produced can be determined through stoichiometry, using the provided balanced chemical equation and molarity (M) of the acetic acid HC2H3O2. According to the balanced chemical equation, one mole of NaHCO3 reacts with one mole of HC2H3O2 to produce one mole of CO2. In other words, the moles of HC2H3O2 used equals the moles of CO2 produced.
First, calculate the moles of HC2H3O2 by multiplying the given volume (0.100 L) by its molarity (0.83 mol/L): 0.100L x 0.83 mol/L = 0.083 mol.
So, according to the stoichiometric ratio, 0.083 mol of HC2H3O2 would produce 0.083 mol of CO2. If you want your answer in grams, note that the molar mass of CO2 is approximately 44.01 g/mol. Multiply the moles of CO2 by its molar mass: 0.083 mol x 44.01 g/mol = 3.65g.
So, the amount of CO2 produced would be 3.65 grams.
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c. turning lithium into fluorine.
b. losing or gaining protons.
d. losing or gaining electrons.
3. Two factors that determine whether a molecule is polar are the types of atoms in the molecule and the ____________________ of the molecule.
4. According to John Dalton’s observations, when elements combine in a compound
A. The ratio of their masses is always the same.
B. Each element contributes an equal number of atoms.
C. Their volumes are always equal.
D. Their masses are always equal.
5. Democritus thought that matter was made of tiny particles
A. Of earth, air, fire, and water.
B. That could not be divided.
C. That could be divided.
D. That were all round and smooth
6. Rutherford’s gold foil experiment provided evidence for which of the following statements?
A. Negative and positive charges are spread evenly throughout an atom.
B. Alpha particles have a positive charge.
C. Gold is not as dense as previously thought.
D. There is a dense, positively charged mass in the center of an atom.
7. Which statement about subatomic particles is true?
A. Protons, neutrons, and electrons all have about the same mass.
B. Unlike protons or neutrons, electrons have no mass.
C. Neutrons have no charge and no mass.
D. An electron has far less mass than either a proton or neutron.
8. Which statement is true about oxygen-17 and oxygen-18?
A. They do not have the same number of protons.
B. Their atoms have an identical mass.
C. They are isotopes of oxygen.
D. They have the same mass number.
9. Which statement accurately represents the arrangement of electrons in Bohr’s atomic model?
A. Electrons vibrate in fixed locations around the nucleus.
B. Electrons travel around the nucleus in fixed energy levels with energies that vary from level to level.
C. Electrons travel around the nucleus in fixed energy levels with equal amounts of energy.
D. Electrons travel randomly in the relatively large space outside the nucleus.
10. What does the electron cloud model describe?
A. The most likely locations of electrons in atoms
B. The precise locations of electrons in atoms
C. The number of electrons in an atom
D. The mass of the electrons in an atom
11. What is the difference between an atom in the ground state and an atom in an excited state?
A. The atom in the ground state has less energy and is less stable than the atom in an excited state.
B. The atom in an excited state has one fewer electron than the atom in the ground state.
C. The atom in an excited state has more energy and is less stable than the atom in the ground state.
D. The atom in an excited state has one more electron than the atom in the ground state.
12. The usefulness of Mendeleev’s periodic table was confirmed by
A. the discovery of subatomic particles.
B. its immediate acceptance by other scientists.
C. the discovery of elements with predicted properties.
D. the discovery of the nucleus.
13. Atoms of the most reactive elements tend to have
A. one or seven valence electrons.
B. eight valence electrons.
C. four or five valence electrons.
D. no valence electrons.
This answer explains chemical concepts related to the periodic table, atomic theory, the nature of molecules, and properties of subatomic particles.
1. Mendeleev organized elements in his periodic table in order of increasing atomic mass.
2. You would select the compound with the highest melting point as the ionic compound.
3. The types of atoms in the molecule and the shape of the molecule determine whether a molecule is polar.
4. According to Dalton, The ratio of their masses is always the same when elements combine in a compound.
5. Democritus thought that matter was made of tiny particles that could not be divided.
6. Rutherford’s gold foil experiment provided evidence that there is a dense, positively charged mass in the center of an atom.
7. It’s true that an electron has far less mass than either a proton or neutron.
8. Oxygen-17 and oxygen-18 are isotopes of oxygen.
9. In Bohr’s atomic model, electrons travel around the nucleus in fixed energy levels with energies that vary from level to level.
10. The electron cloud model describes the most likely locations of electrons.
11. An atom in an excited state has more energy, and is less stable than an atom in the ground state.
12. The usefulness of Mendeleev’s periodic table was confirmed by the discovery of elements with predicted properties.
13. Atoms of the most reactive elements tend to have one or seven valence electrons.
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