stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
Chemistry Semester 1 Review Flashcards | StudBud
Explore
/
Chemistry Semester 1 Review
Chemistry Semester 1 Review
50 terms
·
StudBud Administration
·
4,897 plays
Review of high school chemistry semester one
Flashcards
50 cards
F
Practice quiz
P
Host live
L
Questions
50
Answers
1
Which type of compounds generally have the lowest melting and boiling points?
ionic
metallic
molecular
network covalent
2
What is the density of a nugget of gold with mass of 100g and volume 5.18 cm
3
?
518 g/cm3
12.6 g/cm3
10 g/L
19.3 g/cm3
3
My balance read 16.3 g but the actual mass is 16.5 g. What is my percent error?
24%
1.2 %
10%
12%
4
Which rule states that an orbital may describe at most 2 electrons with opposite spins?
Pauli Exclusion Principle
Heisenberg's Uncertainty Principle
Hund's Rule
Aufbau Principle
5
A reaction occurs and the products are different from the reactants, it is a _______________.
physical change
chemical change
6
What is the frequency of light with a wavelength of 6 X10
-4
m?
1.8 X 105 s-1
2.998 X 108 m/s
5 X 1011 s-1
55 s-1
7
What do the first and second arrow tell you about oxygen?
symbol and element name
atomic number and mass
atomic number and symbol
Symbol and mass
8
What is the correct formula for the ionic compound made of potassium and sulfur?
K2S
K3S2
KS
KS2
9
Multiply 13.05 X 4.3 and express your answer to the correct number of significant figures.
56
56.1
56.11
56.115
10
Compared to the other two subatomic particles, which is completely true of the electron?
neutral, heaviest particle
negative charge, smallest particle
positive charge, smallest particle
positive charge, largest particle
11
How does carbon-12 differ from carbon-13?
one less neutron
one less electron
One less proton
There is no difference
12
What is the most electronegative element?
Helium
Fluorine
Cesium
Hydrogen
13
Express 10.06798 in three significant figures.
10.0
10.067
10.1
10
14
Use VSEPR theory to predict the shape of NH
3
.
tetrahedral
linear
trigonal planar
trigonal pyramid
15
Which of the following is not a traditional area of study in chemistry?
analytical
physical
inorganic
nanotech
16
Identify each type of alloy in the picture.
a- interstitial b- substitutional
a- interstitial b- bimetallic
a- substitutional b- interstitial
a - ionized b-neutral
17
The substances formed after any chemical reaction occurs are called _______________.
ashes
reactants
products
compounds
18
Which is an extensive property?
density
specific heat
heat
volume
19
The valence electrons in metals are modeled as this.
shared between two atoms
locally attached to each atom
a sea of electrons
detached from the metal
20
When a mixture is uniform throughout, it is called a ____________________.
heterogenous mixture
compound
pure substance
homogeneous mixture
21
Convert from 55.4 m/s to km/min.
3.32 X 106
3.32
1012
9.23 X 10-4
22
Electron sharing occurs in molecules to give them the electron configuration of what elements?
halogens
noble gases
alkali metals
metalloids
23
Correctly interpret this formula as to the elements it contains: H
2
SO
4
a weak acid
two hydrogens, one sulfur and four oxygen atoms
two sulfur and four oxygen atoms
hydrogen and sulfur
24
Where are nonmetals located on the periodic table?
below the main table
upper right
lower left
middle
25
Which of the following is not a polar molecule?
CO
HF
H2O
CH4
26
Which is the correct electron configuration for Nitrogen?
1s22s22p3
1s22s22p6
1s22p3
1s22s22p2
27
Which is
not
a property of ionic compounds?
malleable
high boiling point
good conductor when melted or dissolved
brittle when struck
28
How many valence electrons does Selenium have?
4
6
2
8
29
How many significant figures are in 207.0010
7
5
6
3
30
What is 20 degrees Celsius expressed in Kelvin?
293K
-253K
0K
53K
31
Who drafted the first scientific atomic theory in the late 18th century?
JJ Thomson
John Dalton
Democritus
Ernest Rutherford
32
Which is a
basic
unit of measurement in the SI system?
calorie
pound
second
liter
33
Transition metals have unfilled orbitals in which block?
s
f
d
p
34
When a neutral atom loses electrons, what is formed?
a polyatomic ion
a cation
a neutral atom of another element
an anion
35
Which letter identifies spherical orbitals?
f
s
d
p
36
Which is not a state of matter?
solid
liquid
gas
air
37
Which element has the greatest electron shielding of its valence electrons?
K
Cs
Rb
Na
38
To express that my measurement is 10
-9
times the base unit, which prefix do I use?
milli
nano
Mega
micro
39
Which of the following is a chemical formula?
Ar
CO
Be
Se
40
4 g of H react completely with 12 g of carbon, how much methane (CH
4
) will form?
32g
2g
6.02 X 1023 g
16 g
41
What is a proposed explanation for an observation?
experiment
theory
scientific law
hypothesis
42
What is the crystal arrangement of the picture on this page?
face centered cubic
body centered cubic
hexagonal close packed
primitive cubic
43
How does atomic size change from left to right across a period of the periodic table?
increases
stays the same
increases and then decreases
decreases
44
Which correctly describes the composition of cesium-133?
55 p+, 54 e-, 133n0
55 p+, 55 e-, 133n0
133 p+, 133 e-, 133n0
55 p+, 55 e-, 78 n0
45
This is not a clue that a chemical change has occurred.
formation of a precipitate
change in size
production of a gas
heat gained or lost
46
What does Te represent when you see it on the periodic table?
tellurium
technetium
thorium
titanium
47
Which is a chemical property?
ability to combust
boiling point
melting point
color
48
How did Mendeleev arrange the elements in his periodic table?
color, light to dark
atomic number
most reactive last
atomic mass
49
How many sublevels are at the fourth principal energy level?
3
8
1
4
50
What is the weakest type of intermolecular attraction?
dispersion
hydrogen bond
dipole-dipole
ion-dipole
