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Topic 2 Atomic Structure Flashcards | StudBud
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Topic 2 Atomic Structure
Topic 2 Atomic Structure
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Chemistry for IB #IB
Flashcards
22 cards
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Questions
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Answers
1
Which statement is correct about the isotopes of an element?
They have the same mass number.
They have more protons than neutrons.
They have the same electron arrangement or configuration
The same numbers of protons and neutrons in the nucleus.
2
Which is an incorrect statement about atomic emission spectrum of hydrogen?
Frequency lines depend on the difference of energy levels
It is a continuous spectrum
The spectrum consists of several series of lines
Electronic transitions n=2 rise lines in the visible region
3
An element has the electron arrangement 2,8,6. What is the element?
Ar
P
S
C
4
What is the correct number of each particle in a fluoride ion,
19
F
-
?
Protons=9, Neutrons=10, Electrons=10
Protons=9, Neutrons=19, Electrons=9
Protons=9, Neutrons=10, Electrons=8
Protons=9, Neutrons=10, Electrons=10
5
Which of the following atoms has the greatest number unpaired electrons in the ground state?
Fe
Ni
Mn
Sc
6
An element consists of 2 isotopes:72% of mass # 85 and 28% of mass # 87. What is the range?
between 86 and 87
more than 88
between 85 and 86
less than 85
7
X has the electron arrangement 2, 8, 6. Name the chemical species most likely to be formed?
the compound XF8[X8+8F-]
The ion X3+
the ion X6+
the compound H2X[2H+X2-]
8
Which electronic transition within a hydrogen atom requires the greatest energy?
n = 2 → n = 3
n = 1 → n = 2
n = 5 → n = ∞
n = 3 → n = 5
9
Which one of the following statements is true?
The chlorine-35 and Cl-37 atoms are present in equal amount
The ratio of chlorine-37 atoms to chlorine-35 atoms is 2 : 1
The ratio of chlorine-37 to cholrine-35 atoms is 37/35
There are 3 times as many chlorine-35 atoms as Cl-37 atoms
10
Which one of the following atoms will have the same number of neutrons as an atom of
88
38
Sr
8737 Rb
8938Sr
8436Kr
9139Y
11
What does an atomic orbital in an atom represent?
Distance from the nucleus where an electron is always found.
An electron moving around the nucleus of an atom.
A region of space were is probable to an find an electron.
A point of zero electron density.
12
How many valence electrons(in the outermost shell) are present in the element of atomic mass?
1
3
4
2
13
Which of the following particles contains more electrons than neutrons?
II and III only
I and II only
I only
II only
14
All isotopes of uranium have the same A)number of protons; B)number of electrons; C)mass number
C only
A and C only
B only
A only
15
What information abpout the strusture of a helium atom can be gained from it emition spectrum?
The electron in the helium atom are held near the nucleus.
The electrons may exist in any of several energy levels.
A helium atom contains two electrons and two protons
Most of the mass of the atom is in its nucleus.
16
Why was Bohr theory of the atom developed?
To the ratios by mass of elements in compounds
To the emission or line spectrum of hydrogen atoms
To account for chemical formulas
To changes in gas volume with temperature
17
Which of these atomic orbital descriptions is not allowed under modern orbital theory?
5p
2d
4s
4f
18
Which atatement is correct about a line emission spectrum?
e- absorb energy as they move from + to - energy levels (EL)
e- neither absorb nor release E as they move from - to + EL
e- release energy(E) as they move from + to - energy levels
e- release energy (E) as they move from - to + energy levels
19
These are atomic numbers and mass numbers for 4 different nuclei. Which two are isotopes?
I and II
III and IV
I and IV
II and III
20
How many unpaired e- are present in an atom of element with a p (Z) of 23 in its ground state?
3
5
1
7
21
Which statement is correct for the emission spectrum of the hydrogen atom?
In visible regions electron transition close to the nucleus
The line to the best emission is in the ultraviolet region
Lines produce when electrons move from lower to higher level
The lines converge at lower energies
22
Which elements are charaterized by the filling of d orbitals?
halogens
actinides
first row transition series
rare earths (lanthanides)
