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First Semester Chemistry Review Flashcards | StudBud
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First Semester Chemistry Review
First Semester Chemistry Review
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General chemistry concepts as would be encountered in regular level high school chem class.
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50 cards
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1
More than one correct Lewis structure representation of a molecule:
resonance structures
empirical formulas
coordination structures
structural formulas
2
Light of sufficient energy (frequency) striking a metal will cause electrons to be ejected:
quantum leap
photo-activation
emission spectrum
photoelectric effect
3
The strongest intermolecular forces:
Dipole-Dipole interactions
Ionic Bond
Covalent Bond
van der Waals forces
4
A process in which substances are changed into different substances is a:
distillation
chemical reaction
miracle
separation
5
According to VSEPR theory, a water molecule has a "bent" shape due to:
Dipole-dipole interactions
The polarity of its bonds
Van der Waals forces
Repulsive forces between unshared pairs of electrons
6
The energy required to remove an electron from an atom in the gaseous state is the:
quantum
periodic law
ionization energy
electronegativity
7
A measurement which is very close to its TRUE value is said to be:
reproducible
Precise
Estimated
Accurate
8
The measurement, 1042 L, rounded off to three significant figures is:
1.05X 103 L
1.01 X 103 L
1040 L
1050 L
9
<p>Energy required to move an electron to next higher energy level:</p>
photon
quantum
wavelength
spectrum
10
Which area of the periodic table contains elements with "d" orbitals being filled?
Noble gases
Inner transition metals
Transition metals
Alkali metals
11
Determine the type of bond formed between two atoms of carbon :
metallic
polar covalent
nonpolar covalent
ionic
12
How many electrons does an atom of Cu(I) have?
30
28
27
29
13
Which electrons participate in intramolecular bonding?
excited state electrons
ground state electrons
core electrons
valence electrons
14
Ability of an atom to attract electrons to itself when it's bonded to another atom:
photoelectric effect
radioactivity
electronegativity
ionization energy
15
A physical blend of two or more components is a(n):
chemical reaction
phase
mixture
substance
16
An exothermic process is one which:
releases energy in the form of heat
consumes more energy than it produces
creates energy
Requires addition of energy
17
Each period in the periodic table corresponds to ________________:
an orbital
a suborbital
an energy sublevel
a main energy level
18
The weakest intermolecular force:
van der Waals Forces
Covalent Bond
Hydrogen Bond
Ionic Bond
19
Which of the following representations of the element (as it appears in nature) is incorrect?
I2
He
O2
H
20
The correct chemical formula for the compound iron (III) phosphide:
Fe3P3
Fe3(PO4)2
FePO3
FeP
21
The correct formula for sodium nitride is:
Na(NO2)
Na3N
NaN3
NaNO3
22
Which type of bond confers the property of brittleness to compounds?
Polar Covalent
Metallic
Covalent
Ionic
23
The density of Cu is 8.92 g/cm
3
. How much volume is occupied by 16 g of Cu?
1.8 L
0.56 cm3
1.8 cm3
142 cm3
24
The correct electron configuration for Mn is:
1s22s22p63p64s23d5
[Ar]4s23d5
1s22s22p63s23p63d5
[Ne]3s23p63d5
25
From the periodic table, determine the number of neutrons in an atom of Silicon:
14
32
28
6
26
Which of the following is NOT a physical change?
salt dissolving in water
water evaporating
sodium metal reacting with water
making an alloy of copper and tin
27
How many distinct phases can be dintinguished in the test tube in the image?
4
2
1
3
28
Which of the following is true about compounds?
They have variable compositions
they have properties similar to their component elements
They have definite composition
They can be physically separated into component elements
29
The smallest particle of a covalent compound is a(n):
molecule
ion
formula unit
isotope
30
Representation of kind and number of atoms in a compound.
chemical formula
chemical equation
product
reactant
31
Which subatomic particle determines the chemical properties of an atom (element)?
Proton
Nucleus
Electron
Neutron
32
Convert 0.40 kg to g using correct significant figures:
4 X 103 g
400. g
4000 g
4.0 x 103 g
33
Determine the mass number for an atom of C which has 8 neutrons:
14
6
8
12
34
Which of the following is a transition element?
tin
Aluminum
Copper
cesium
35
Which of the following atoms would be largest?
Cs
S
Ba
Li
36
The name of this compound: Cu(NO
3
)
2
Copper (I) Nitrite
Copper (II) Nitrate
Copper Nitrate
Copper Nitrite
37
Which of the following atoms has the least attraction for electrons when bonded?
As
N
Fe
Cl
38
Which of the following compounds is molecular (covalent)?
C6H12O6
MgO
Na2SO4
KCN
39
How many protons does a sulfur ion have?
18
14
16
15
40
Which of the following properties is conferred by a metallic bond?
Crystalline Latice
Malleability
Brittleness
Ultra Low Melting Point
41
How many electrons would an ion of Calcium have?
20
18
40
22
42
What is the volume of 10 g of mercury metal (density ~8 g/cm
3
)?
0.8 mls
1.25 mls
8 mls
80 mls
43
Which of the following electron ?onfigurations represents an alkaline earth metal
1s22s22p63s23p6
[Ar]4s23d5
[Ne]3s23p64s1
1s22s22p63s2
44
I-131 is an example of a(n):
molecule
Ion
Isotope
formula unit
45
When an electron falls from a higher energy level to a lower energy level:
energy is absorbed
a photon may be released
the atom collapses
a photon may be absorbed
46
A horizontal row in the periodic table.
group
period
block
family
47
A metalloid in the fourth period of the periodic table:
Si
B
Ge
Ga
48
Which of the following instruments has the highest precision?
cg balance
a kg balance
g balance
ug balance
49
Which of the following elements has the greatest first ionization energy?
O
Na
Ca
S
50
A covalent bond occurs when:
two atoms share one or more electrons
dipole-dipole interactions occur
oppositely-charged ions attract
like-charged ions attract
