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Practice questions on various topics related to atomic particles, universal forces, and chemical bonding. The questions cover identifying subatomic particles, matching them with their descriptions, understanding the role of universal forces, and ranking molecules based on their boiling points and intermolecular forces. Students can use these questions to test their knowledge and prepare for exams.
Typology: Lecture notes
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Practice Questions
Topic 1
For questions 1-9, match the description with the correct sub atomic particle(s)
a. Electron b. Proton c. Neutron d. Proton & neutron e. Proton & electron
chemical bonding between atoms
charge
questions 19-23--there is no answer for # For questions 10-22, match the universal force with its role. Note the numbering error--- should be 19 through 2 2.
Topic 2 questions
Use the table to the right to answer questions 28 & 29
points? a. H 2 O N 2 O 2 He b. N 2 H 2 O He O (^2)
c. He H 2 O N 2 O (^2) d. He N 2 O 2 **H 2 O *****
a. H2O N2 O2 He b. N2 H2O He O
c. He H2O N2 O d. (^) He N2 O2 **H2O *****
d. **slow down *****
Figure 1
liquid to a gas you would need to ____________.
**decrease the pressure *****
and/or increase the pressure
and pressure
and the pressure
closely at Figure 2 when choosing your answer).
a solid to a vapor. This process is known as
energy?
higher ionization energy and larger atomic radius. Answers will vary depending on the elements you chose, but that radius increases down, and decreases across. Ionization energy is opposite.
_Ionic bonds form through the transfer of electrons between cations (metals) and anions (non-metals). Their electronegativity difference is ~ greater than or equal to 1. ** Covalent bonds form through the the sharing of electrons between non-metals. Polar covalent bonds show electronegativity difference between 1.69 and 0.4; they display an uneven sharing of electrons. Non-polar bonds show an electronegativity difference less than or equal to 0.4, and evenly share electrons_**
lose when it becomes an ion? Atoms want to gain or lose electrons to stabilize, and the most stable elements are those with full valence shells: the Noble gases. All but Helium have 8 valence electrons, and the prefix for 8 is "oct-", hence the "octet rule." Metals have fewer valence electrons than non-metals, and its "easier" for them to lose electrons to stabilize and take on the electron configuration of the closest Noble gas, which are "behind" them on the periodic table. Non-metals are the opposite, they gain electrons to take on the configuration of the closest Noble gas, which are "in front" of them on the periodic table.
and writing their formula. see answer key for that assignment