Chem Final Review

Question 1

Rules for Counting Significant Figures

1. Nonzero Integers

Answer 1

Nonzero integers are always significant.

Question 2

Rules for Counting Significant Figures

2. Zeros
   a) leading zeros

Answer 2

Leading zeros are zeros that precede all nonzero digits. These do not count as significant figures.

ex. 0.0025 has two sig figs.

Question 3

Rules for Counting Significant Figures

2. Zeros
   b) captive zeros

Answer 3

Captive zeros are zeros between nonzero digits. These always count as significant figures.

ex. 1.008 has four sig figs

Question 4

Rules for Counting Significant Figures

2. Zeros
   c) Trailing zeros

Answer 4

Trailing zeros are zeros at the right end of the number. They are significant only if the number contains a decimal point. The number 100 has one sig fig, 1.00*10^2 has three sig figs.
100. has three sig figs.

Question 5

Rules for Counting Significant Figures

3. exact numbers

Answer 5

this is the 2.54 cm in a inch kind of thing.

Question 6

Rules for Significant Figures in Mathematical Operations

1. For Multiplication or division

Answer 6

The number of sig figs in the result is the same as the number in the least precise measurement used in the calculation.

ex. 4.56*1.4=6.38 –> 6.4

Question 7

Rules for Significant Figures in Mathematical Operations

2. For addition or subtraction

Answer 7

The result has the same number of decimal places as the least precise measurement used in the calculation.

Question 8

Celsius to Kelvin

Answer 8

T(celsius) + 273

Question 9

Celsius to Fahrenheit

Answer 9

T(celsius)*(9/5) + 32

Question 10

Law vs Theory

Answer 10

A law summarizes what happens, a theory is an attempt to explain why.

Question 11

Daltons Atomic Theory 
1
2
3
4

Answer 11

1) each element is made up of tiny particles called atoms
2) the atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways.
3) chemical compounds are formed when atoms of different elements combine with each other. A given compound always has the same relative numbers and types of atoms.
4) Chemical reactions involve reorganization of the atoms - changes in the way they are bound together, atoms not changed.

Question 12

J. J. Thomson experiment

Answer 12

Cathode-Ray, discovered charge to mass ratio of electron

Question 13

Milikan experiment

Answer 13

Oil Drop, discovered charge of electron

Question 14

Rutherford experiment

Answer 14

Gold Foil, atoms have a dense center of positive charge, electrons around, a lot of space

Question 15

c=

Answer 15

lambda*v

Question 16

Using Planck’s constant

∆E=

Answer 16

nhv

Question 17

E(photon)=hc/lambda

Answer 17

hc/lambda

Question 18

principal quantum number (n)

Answer 18

integral values (1,2,3) as n increases, the orbital becomes larger and the electron spends more time farther from the nucleus. 
An increase in n also means higher energy, the electron is less tightly bound to the nucleus

This number is the coefficient so
3s^2, n=3

Question 19

Angular momentum quantum number (l)

Answer 19

integral values from 0 to n-1
Related to the shape of the atomic orbitals. 
l=0, s
l=1, p
l=2, d
l=3, f
l=4, g

Question 20

magnetic quantum number (ml)

Answer 20

Integral values between l and -l, including zero.
Value of ml is related to the orientation of the orbital in space relative to the other orbitals in the atom.

so if it’s 2p, ml -1, 0, +1
4s, 0
3d, -2, -1, 0, 1, 2

Question 21

Electron configuration of copper

Answer 21

[Ar] 4s^1 3d^10

Question 22

Electron configuration of chromium

Answer 22

[Ar] 4s^1 3d^5

Question 23

Trend in atomic radius

Answer 23

fill in

Question 24

Trend in ionization energy

Answer 24

fill in

Question 25

Trend in electron affinity

Answer 25

fill in