Unit 1 Flashcards
Matter
States of matter
Matter: anything that has mass and takes up space
Solid
Liquid
Gas
Diff between physical and chemical changes and properties
Physical properties: describe matter how it exists Shape Color Size Temp
Chem : matter as it changes form (chemicaly) Change in chemical make up of item Cooking Burning Chemical reactions
Law of the conservation of mass
Mass is neither created or destroyed in a chemical reaction
Elements v compounds v pure substances
Mixtures ( homogenous v heterogeneous)
Pure substances : same physical and chemical properties throughout
Reped by chem formula
Mixture : matter with variable composition
More then one substance (physical)
Element : cannot be broken down into simpler pure substance
Compound : 2 or more elements
Alloy: homogeneous mixture of a base metal
Solution= homogeneous mixture
Metals v non metals v semimetals
Metals Solid room temp Shiney Conductor Heat well Malleable Ductile
Nonmetals Brittle Insulator Does not heat well No shiney sheets or wires Not all solid at room temp
Semi metals
Have properties of both
Sig fig rules 🤮
+- is to lowest place
*\ is lowest # sigfigs
Volume v area v density
Volume= lengths * widths * heights
M^3
1 ml = 1 cm^3
Area = length times width
M^2
Density = mass\volume
Fahrenheit to Celsius
C=(F-32) * 5/9
Celsius to Fahrenheit
F= (C*9/5)+32
Celsius to kelvin
Kelvin = C +273.15
Kelvin to Celsius
C=k-273.15
Isotope
Symbolic notation
Isotope - atoms of same element same proton but different neutrons
A/z X
A -atomic mass
Z- atomic number
X - symbol
Metals v metalloids v non-metals
Metals - left of zig zag
Non - right of zigzag
Semi - br si ge as at te
Transition and inner transition (metals location)
Representative
Rep elements 1A to 8a
Most common
Transitional are b group (1b to 8b)
Transitional are bottom two rows
Alkali metals
1A
Left column
Alkaline earth metals
2A
And left Column
Halogens
Group 7a
Almost last right column
Noble gases
Group 8a
Right column
Charges formed by groups
1A 2A 3A (Al and Ge) 6a 7a
1A make +1
2A make + 2
3a
6a -2
7a -1
Protons v neutrons v electrons
Protons + nucleus 1 amu
Neutrons () nucleus 1 amu
Electron - basically no amu
Calculate atomic mass from isotopic masses and NATURAL Abundance
Natural abundance * AMU + NA *AMU
Mole
Number of things equal to the number of atoms in carbon 12
Or
1 mol = 6.022*10^23
Mole to mass
Atomic mass in grams = 1 mol
Avogodros number 🥑
6.022*10^23
Period v group / family
Period row
Family column
