Question 1

Two unknown liquids, A and B, were reacted to form a solid C and liquid D. The products of the reaction resemble those of an acid-base reaction. With these observations, can we determine whether liquid A, liquid B, solid C, and liquid D are elements or compounds?

Accepted Answer

No, we cannot tell

Question 2

Is melting an ice cube a physical or chemical process?

Accepted Answer

Physical process

Question 3

Select a chemical property of uranium:

Accepted Answer

Reacts with cold water

Question 4

An unknown element was observed to have the following properties:
1. It appears as a silvery liquid.
2. It has a density of 13.53 g/cm$$^3 at $$room temperature.
3. It reacts with molecular iodine to produce a red solid.
4. It freezes at $$-38.83\ ^\circ\mathrm{C}$$ and boils at $$356.73\ ^\circ\mathrm{C}.
5. It $$forms a yellow solid when combined with dilute nitric acid.
Classify each property as physical or chemical.

Accepted Answer

Physical properties: 1, 2, 4
Chemical properties: 3, 5

Question 5

Select the extensive property from the list below.

Accepted Answer

volume

Question 6

The summit of a mountain has an average temperature of $$13\ ^\circ\mathrm{F}. $$Express the temperature in Kelvin. Use the conversion formulas: $$T_{\mathrm{C}} = \frac{5}{9}(T_{\mathrm{F}} - 32)$$ and $$T_{\mathrm{K}} = T_{\mathrm{C}} + 273.15.$$

Accepted Answer

263 K

Question 7

True or False: To express a number in scientific notation, increasing the coefficient value means the exponent is negative while decreasing the coefficient value means the exponent is positive.

Accepted Answer

False

Question 8

In classical mechanics, kinetic energy is defined as $$\frac{1}{2}mv^2$. Derive a unit for energy starting with SI base units. Using SI prefixes, suggest a convenient unit for the kinetic energy of a car weighing 2500 pounds moving at 45 mi/hr and the kinetic energy of an electron moving at 35% of the speed of light (m_e = 9.11$$ 	imes $$10^{-31} kg$$, $$c = 3.00 	imes 10^8$ m/s).

Accepted Answer

J; kJ; fJ

Question 9

What is the equivalent value of 513 mK/s in K/s?

Accepted Answer

0.513 K/s

Question 10

Determine the number of significant figures in the following scientific notation: $$2.71 	imes 10^5$.

Accepted Answer

3

Question 11

A vehicle's speedometer is shown below. What is its reading in km/hr and mi/hr? How many significant figures should the reading have?

Accepted Answer

115 mph with 3 significant figures and 185 kmh with 3 significant figures

Question 12

Perform the following operation. Express the answer using the correct number of significant figures: $$780 + 6.97 - 81.197.$$

Accepted Answer

705.8

Question 13

Is a fluid ounce larger than a pint? By how much?

Accepted Answer

No, a pint is about 16 times larger than a fluid ounce.

Question 14

The nitrogen level in an urban apartment is $$521\ \mu\mathrm{g}/\mathrm{m}^3. $$Calculate the mass of nitrogen gas in grams if the urban apartment is $$10.2\ \mathrm{ft} 	imes 9.8\ \mathrm{ft} 	imes 21.5\ \mathrm{ft} in $$dimension. ($$1\ \mathrm{ft} = 0.3048\ \mathrm{m})$$

Accepted Answer

2.1 g

Question 15

A student needs cyclohexane for an experiment. They measured 15 mL of the liquid and found that it weighs 26.2 g. A chemistry textbook listed cyclohexane to have a density of $$0.773\ \mathrm{g/mL} at $$room temperature. Is it possible that the liquid is cyclohexane?

Accepted Answer

No

Question 16

The diameter of a spherical ball of copper is $$3.95\ \mathrm{cm}. If $$the density of copper is $$8.96\ \mathrm{g/cm}^3$$, determine the mass of the sphere. Use $$V = \frac{4}{3}\pi r^3$ to calculate the volume of a sphere, where r$ is the radius.

Accepted Answer

376 g

Question 17

An aluminum bicycle frame weighing $$3.69\ \mathrm{kg}$$ was placed in a pool filled with water. The displaced water was measured to be $$1.365\ \mathrm{L}. $$Calculate the density of the metal. ($$1\ \mathrm{L} = 1000\ \mathrm{cm}^3)$$

Accepted Answer

2.70 g/cm$$^3$$

Question 18

Identify the element that 'X' represents in $$^{72}_{32}X.$$

Accepted Answer

germanium

Question 19

Determine the heavier atom between $$^{14}\mathrm{C}$$ and $$^{14}\mathrm{N} by $$comparing the total masses of their subatomic particles.

Accepted Answer

$$^{14}\mathrm{C} is $$heavier than $$^{14}\mathrm{N}$$

Question 20

If six electrons were removed from tungsten, $$^{184}\mathrm{W}$$, write the symbol of the ion formed.

Accepted Answer

$$^{184}\mathrm{W}^{6+}$$

Question 21

There are two stable isotopes of chlorine, $$^{35}\mathrm{Cl}$$ and $$^{37}\mathrm{Cl}$$. $$^{35}\mathrm{Cl}$$ has a mass of $$34.9689$$ amu and a natural abundance of $$75.77\%. $$Calculate the m/m % of $$^{37}\mathrm{Cl}$$ which is the mass of $$^{37}\mathrm{Cl} in $$grams contained in 100 grams of chlorine element.

Accepted Answer

24.23 %

Question 22

Classify the following as metal or nonmetal: Na, Br, N, Ca.

Accepted Answer

Na = metal; Br = nonmetal; N = nonmetal; Ca = metal

Question 23

Identify the group name for each element: Ba, Cl, Ne, Na, At.

Accepted Answer

Ba = alkaline earth metal; Cl = halogen; Ne = noble gas; Na = alkali metal; At = halogen

Question 24

Determine if vanadium is a main-group element or not.

Accepted Answer

Vanadium is in group 5B so it's not a main-group element.

Question 25

Name the following elements with the symbols: Rh, Si, O, P.

Accepted Answer

Rhodium, Silicon, Oxygen, Phosphorus

Question 26

Visualize elements X and Y as described:
• Element X (atomic element): Atoms represented by triangles.
• Element Y (diatomic molecular element): Atoms represented by squares.
Which image best represents this description?

Accepted Answer

Image 2: X is single atoms (triangles), Y is paired squares (diatomic molecules)

Question 27

At standard conditions, some elements only exist as solids. Is this statement true or false?

Accepted Answer

True

Question 28

Identify which among the elements given below loses or gains electrons.
A. Pb
B. Al
C. N
D. I

Accepted Answer

Al and Pb are expected to lose electrons while I and N are expected to gain electrons.

General Chemistry 1 Midterm Study Guidance – Part 1

Study Guide - Practice Questions

Study Guide - Flashcards