Semester 2 Review Flashcards
What does temperature measure?
The average kinetic energy of particles in a sample of matter
Explain what is meant by the terms exothermic and endothermic
Exothermic is when a substance gives off heat, endothermic is when a substance absorbs heat.
What is meant by the specific heat capacity of a material?
Specific heat is the amount of heat required to raise the temp of one gram of that substance to 1 degree C
Calculate the mass (in grams) of each of the following substances that could be warmed over the indicated
temperature range by application of exactly 1.0 kJ of energy. (1.0 kJ = 1000J)
a. water, from 15°C to 42°C s=4.184 J/g °C
b. iron, from 25°C to 125°C s=0.45 J/g °C
c. carbon, from -10°C to 47°C s=0.71 J/g °C
a. 1000J/(4.18427°C)=8.85gH2O b. 1000J/(.45100°C)=22.2gFe
c. 1000J/(.71*57°C)=24.7gC
How many s,p,d and f orbitals can occupy any given energy level?
S-1, P-3, D-5, F-7
How many electrons can occupy an orbital at any given energy level?
2 electrons per orbital
What is the shape of a p-orbital? S-orbital?
P orbital- dumbbell shaped
S orbital- sphere shaped
What is the lowest energy level that can have a p-orbital? D-orbital? F-orbital?
P-orbital level 2
D-orbital level 3
F-orbital level 4
Is it possible for two electrons in the same atom to have exactly the same set of quantum numbers?
No, no two electrons can have the same quantum numbers
When is an electron configuration considered stable
When the subshells are full
Distinguish between an atom in its ground state and an excited atom
An atom in ground state had the lowest possible energy and an atom in excited state has gained energy
What happens when a photon of light is emitted?
A photon of light emits when an electron goes from excited states back to ground state
For the following elements list the electron configuration.
a. oxygen, cesium, krypton, titanium, scandium, nitrogen, chlorine
a. oxygen [He]2s2 2p4
1 cesium [Xe]6s
2 10 6 krypton [Ar]4s 3d 4p
22 titanium [Ar]4s 3d
21 scandium [Ar]4s 3d
23 nitrogen [He]2s 2p
25 chlorine [Ne]3s 3p
Define electronegativity
Electronegativity is the ability of an atom to attract electrons
Does electronegativity increase or decrease as the atomic number of an element increases within the same
period of the periodic table?
Electronegativity increases as atomic number increases. It increases from left to right across the periodic
table.
How is the strength of a bond between two elements in a molecule related to their electronegativities?
If the difference in electronegativities of two different atoms is very big, they will have a strong bond. If
the difference in electronegativities is very small, they will have a weaker bond.
What is the difference between an ionic and a covalent bond?
An ionic bond is between a metal and a non-metal. Great electronegativity difference.
A covalent bond is
between two non-metals. Very small electronegativity difference
Referring to the table of electronegativities, classify each of the following bonds as either ionic (I) or
covalent (C):
a.Al-Of
b. Al-S
c. Bi-Cl
d. Bi-O
e. C-Cl
f. N-O
g. Na-S
h. P-O
i. S-O
j. Ti-Br
k. Ca-F
l. Ba-S
Ia.Al-O Cb.Al-S Cc.Bi-Cl Cd.Bi-O Ce.C-Cl Cf.N-O Ig.Na-S Ch.P-O Ci.S-O I j.Ti-Br Ik.Ca-F Il.Ba-S
What atoms forms diatomic molecules
Br2 I2 N2 Cl2 H2 O2 F2
Give an example of a polar covalent and a non polar covalent molecule
Polar covalent-two different atoms C-H
Non-polar- same atom N=N
What does VSEPR stand for?
Valance Shell Electron Pair Repulsion
What does the VSEPR theory predict?
It predicts the shape of molecules
Draw the Lewis dot structure for SiO2
O=Si=O
Convert 1.20 atm to units of mmHg, torr and pascals
1.20 atm * 760mmHg/1atm = 912 mmHg 1.20 atm * 760 torr/1atm = 912 torr
1.20 atm * 101,325 Pa/ 1atm= 121590 Pa
