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YSU / Chemistry / CHEM 41310 / How many moles in 4 g of hydrogen ?

How many moles in 4 g of hydrogen ?

How many moles in 4 g of hydrogen ?

Description

School: Youngstown State University
Department: Chemistry
Course: General Chemistry
Professor: Ken adair
Term: Fall 2018
Tags: General Chemistry
Cost: 50
Name: Midterm 1 Study Guide
Description: Chapter 1 2 and 3 main points and ideas Basic Subatomic and naming of molecules Basic chemistry experiments
Uploaded: 09/26/2018
4 Pages 32 Views 2 Unlocks
Reviews


Element- A atom that cannot be divided, Pure Substance Ex: Tin


How many moles in 4 g of hydrogen ?



Compound- A molecule that can be divided by chemical reaction. Ex: Water (H2O)

Homogenous Mixture- A mixture that is the same composition throughout. Ex: Kool-Aid

Heterogenous Mixture- A mixture that is of varied composition. Ex: Air

Units you must know:

∙ Nano- 1*10 ^-9 ∙ Milli-1*10^-3 ∙ Centi-1*10^-2 ∙ Kilo-1*10^3 ∙ Length= meters

∙ Mass= kg

∙ Temp= kelvin C or F

∙ Time=seconds

∙ Amount=Moles

∙ Dimensional analysis: 


What is dimensional analysis physics?



∙ How many moles in 4 g of Hydrogen ?  


How are isotopes named?



We also discuss several other topics like What are the indefinite articles?

If you want to learn more check out What is archaeological fieldwork?

∙ PS ) always make sure units cancel

∙ Temperature Conversions:

∙ C=(5*c/9*f)*(f—32*f)

∙ F=(9*f/5*c)*(C+32*c)

∙ Sig figs

∙ All non-zero values are significant

∙ Zero is significant if it is between 2 significant values

∙ Zero is not significant if it is leading all numbers

∙ Zero is sig. if tailing all numbers after decimal Don't forget about the age old question of How do we find the certainty equivalent?

∙ exact numbers have infinite sig figs

∙ Atomic Theories

∙ Millikan’s Oil Experiment 1909- Millikan atomized oil drops into a barrel and let them fall in between two charged plated. He then calculated the charge needed to suspend the drops and found the mass and charge of an electron.

∙ Rutherford’s Gold foil 1919- Rutherford sent radiation through a foil of gold. Because the radiation waves mostly went through the foil and didn’t bounce off as expected it disproved the plum pudding theory and proved the nucleus.

∙ Marie Curie & Henri- Radioactivity 1896-1898- They produced radioactive wavelengths by using lead and separated it by using charged plates. This proved the existence of an +and- part of an atom.

∙ Thompsons Cathode ray 1897- Thomson used + and – charges plates to bend the light in a cathode ray tube and measure the charge of an electron.

∙ Calculate # of protons electrons and neutrons in an ion

Don't forget about the age old question of What is tonicity and how does it relate to osmosis?

∙ Charge of an ion

∙ Ions are made of metal

∙ Use group charges  

∙ Cations are +  

1. Use name the add “ion” ∙ Don't forget about the age old question of How does the depiction of vodun feed racist stereotypes of africans?
We also discuss several other topics like What is telencephalon and diencephalon?

∙ Anions are –

1. Use name then add  “ide” then add “ion”

∙ Naming isotopes

∙ Isotopes are the name element with different masses due to differing  amount of neutrons

∙ Add the protons and neutrons to get the name  

∙ Ex: Carbon 12 (6 protons+ 6 neutrons)

∙ Periodic table

∙ Demetri Mendelu 1869 originated by organized mass ∙ Rows by atomic #

∙ Columns have similar properties

∙ Column 1 alkali 1+

∙ Column 2 alkaline 2+

∙ Column 3 2-

∙ Column 4 4-

∙ Column 5 3-

∙ Column 6 2-

∙ Column 7 halogens 1-

∙ Column 8 Nobel Gas 0

∙ Naming acids

∙ If no Oxygen ∙ If Oxygen

∙ Use anion name without  ∙ “ide” and Add “ic”

∙ If “ate” then “ic” ∙ If “ite” then “ous“

∙ Percent composition

∙ Find mass of desired percent divide by total mass and multiply by 100 ∙

∙ Writing and balancing

∙ Multiply each molecule by whatever factor makes both sides possess the  same amount of atoms

∙ Make sure to study stoichiometry ( finding the amount of product yield in a given reaction)

∙ Product yield

∙ Divide the actual yield over the theoretical and multiply by 100 ∙

∙ Patterns of chemical reaction

∙ Displacement

∙ Combination

∙ Decomposition

∙ Precipitation

∙ Combustion

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