1.The Bohr model of the hydrogen atom is
best described as:
1. A large lump of chocolate chip cookie
dough with electrons as the chocolate chips;
those of higher energy are on the outside surface
of the lump
2. Similar to Saturn with electrons of varying
energies in a single circular ring orbiting
around a huge nucleus
3. A minature solar system in which electrons
occupy specific orbits; larger orbits are
occupied by higher energy electrons
4. A loosely packed assortment of subatomic
particles of varying energies; the whole
collection is shaped like a bagel
2.Neils Bohr’s model of the hydrogen atom
explained the unique set of spectral emission
or absorbtion lines seen for hydrogen or other
atoms. Pick the statement that best summarizes
the model.
1. The electrons all formed one single continuous ring around the nucleus. When light
was shone at the atom, this ring expanded.
Because the electrons were further apart and
higher in energy, light was absorbed as this
happened. The color of light absorbed was
related to the number of electrons in the ring.
2. As the hydrogen atom only had one electron,
it only emitted certain colors of light as
it orbited around the nucleus. Larger atoms
had more electrons so more colors were seen.
3. The electrons occupied discrete circu-lar orbits; closer orbits were lower in energy.
Emission lines were caused by electrons in
excited atoms jumping from outer orbits to
closer orbits. Each jump corresponded to a
specific amount of energy released.
4. The electrons were trapped inside the
nucleus and specific amounts of energy (specific
colors of light) were needed to release
them. This varied from one element to another.
3Select the set of bonds below that lists in
order an ionic bond, polar covalent bond, and
and a nonpolar covalent bond.
1. Na-S, N-H, Br-Br
2. Br-Br, N-H, Na-S
3. N O, O-H, N-H
4. Na-S, Br-Br, N-H
5. K-O, H-F, N-H
yf7f
ugi
ujg]
ug
http://www.chemistry.about.com › … › Chemistry Articles & Features
Try also: http://www.en.wikipedia.org/wiki/Bohr_model
1 2 3
2.Neils Bohr’s model of the hydrogen atom
explained the unique set of spectral emission
or absorbtion lines seen for hydrogen or other
atoms. Pick the statement that best summarizes
the model
1.2
2.4
3.1
1. The Bohr model of the hydrogen atom is best described as: 3. A miniature solar system in which electrons occupy specific orbits; larger orbits are occupied by higher energy electrons.
To arrive at this answer, we can eliminate options 1, 2, and 4 as they do not accurately describe the Bohr model. The Bohr model compares the arrangement of electrons in an atom to that of a miniature solar system, where electrons occupy specific orbits around the nucleus. Additionally, larger orbits correspond to higher energy levels for the electrons. This model helps to explain the discrete energy levels and spectral lines observed in the hydrogen atom.
2. Neil Bohr's model of the hydrogen atom: 3. The electrons occupied discrete circular orbits; closer orbits were lower in energy. Emission lines were caused by electrons in excited atoms jumping from outer orbits to closer orbits. Each jump corresponded to a specific amount of energy released.
To find the correct answer, we need to evaluate each statement in relation to Neil Bohr's model. Option 1 is incorrect as it describes a single continuous ring that expands when light is shone. Option 2 is incorrect as it suggests that only one electron emits light, while larger atoms have more electrons emitting more colors. Option 3 aligns with Bohr's model as it describes discrete circular orbits where electrons of lower energy occupy closer orbits. Excited electrons can jump from outer orbits to closer orbits, emitting specific amounts of energy, which corresponds to specific colors of light. Option 4 is again incorrect as it implies that electrons are trapped inside the nucleus, which is not consistent with the Bohr model. Therefore, the correct answer is option 3.
3. The set of bonds that lists in order an ionic bond, polar covalent bond, and nonpolar covalent bond is: 1. Na-S, N-H, Br-Br.
To identify the correct answer, we need to understand the nature of each bond. Ionic bonds occur between a metal and a non-metal, resulting in the transfer of electrons to form charged ions. Polar covalent bonds occur between two non-metals with different electronegativity values, resulting in an unequal sharing of electrons and creating partial charges. Nonpolar covalent bonds occur between two non-metals with similar electronegativity values, resulting in an equal sharing of electrons.
In the given options, Na-S represents an ionic bond as it involves the transfer of an electron from sodium (a metal) to sulfur (a non-metal). N-H represents a polar covalent bond as both nitrogen and hydrogen are non-metals, and nitrogen has a higher electronegativity than hydrogen. Finally, Br-Br represents a nonpolar covalent bond as both bromine atoms share electrons equally due to their similar electronegativity values. Therefore, the correct answer is option 1.