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# Chem Unit 1 Test

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Kayla Timmons

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[Front]

determines the quantity, dimensions, or extent of something
[Back]

measurement

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### Levels:

• 1) Chapter 1   View

### Questions:

155 questions
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 Determines the quantity, dimensions, or extent of something Measurement
 A definite quantity adapted to as a standard of measurement Unit
 How close the measurement is to the "true" value Accuracy
 The degree to which the measurement is reproducable Precision
 A digit that is either reliably known or estimated Significant digit
 How many sig figs are in 1.23 3
 How many sig figs are in 0.0012 2
 How many sig figs are in 0.1100 4
 How many sig figs are in 2500 2
 How many sig figs are in 0.09030 4
 How many sig figs are in 109.0 4
 How many sig figs are in 0.00900 3
 Round this to 3 sig figs: 5345 5350
 Round this to 3 sig figs: 0.01457 0.0146
 Round this to 3 sig figs: 1.053 1.05
 The comparison of the experimental measurement to its accepted value. Percent error
 Cannot be described in terms of anything else. ex: mass=kg, length=m, time=s Fundamental measurement unit
 Fundamental measurements combined to make a derived unit. ex: speed=m/s, density=g/cm^3 Derived measurement unit
 The study of matter and the changes it undergoes Chemistry
 Anything that has mass and occupies space Matter
 The most basic form of matter (ex: silver, gold, copper) Element
 Composed of small indivisible particles called atoms Matter
 Composed of atoms and different elements combined in small whole-number ratios Chemical compounds
 The rearrangement of atoms into different combinations Chemical reactions
 Smallest fundamental particle of an element that has the properties of that element Atom
 The first particle discovered (JJ thompson 1897) Electron
 Electrons have a _______ charge Negative
 + in the nucleus Protons
 0 in the nucleus Neutrons
 - outside the nucleus Electrons
 Number of protons in the nucleus Atomic
 Protons + neutrons Mass number
 Atoms of the same element with differeing mass numbers Isotopes
 Substance composed of two or more elements that are chemically combined (water, table salt, sugar) Compound
 A substance where the atoms are held together by covalent bonds, ex: H2O Molecular compounds
 Compounds consisting of ions (atoms who have gained either a positive or negative charge) Ionic compounds
 Electrostatic forces holding the ions together Ionic bonds
 Charged particle Ion
 Positive charged particle Cation
 Negative charged particle Anion
 Matter is neither created nor destroyed in chemical reactions Law of the conservation of mass
 Solids, liquids, gas Physical states
 Have definite composition and definite unchanging properties Pure substances
 Pure substances tendency to undergo chemical change. ex: burning, color changes, tarnishing Chemical properties
 A substance exists in a particular physical state under defined conditions. increase in temp will alter physical state (ex: color, odor, taste) Physical properties
 Property that does not depend on the amount of material (ex: density) Intensive properties
 Property that does depend on the amount of material present (ex: mass, volume) Extensive property
 When a substance is chemically converted to another substance. Chemical change
 Ratio of mass to volume - an intensive property Density
 Change in physical property (ex: melting, freezing) Physical change
 Non-uniform mixture containing two or more substances (ex: salt and pepper, oil and water) Heterogeneous mixture
 Uniform mixture, same throughout (ex: salt water, milk) Homogeneous mixture
 Substance being dissolved Solute
 Substance doing dissolving Solvent
 The capacity to do work Energy
 Energy cannot be created nor destroyed, but only transformed from one form to another Law of the conservation of energy
 Produce energy Exothermic reactions
 Require energy Endothermic reactions
 Energy availalbe due to position or composition Potential energy
 Energy resulting from motion Kinetic energy
 Amount of heat required to raise the temp of one gram of water from 14.5C to 15.5C Calorie (cal)
 The amount of heat required to raise the temperature of one gram of a substance to one degree celsius (kelvin) - reflects how some substances heat up faster than others Specific heat
 H Hydrogen
 He Helium
 Li Lithium
 Be Beryllium
 B Boron
 C Carbon
 N Nitrogen
 O Oxygen
 F Flourine
 Ne Neon
 Na Sodium
 Mg Magnesium
 Al Aluminum
 Si Silicon
 P Phosphorus
 S Sulfur
 Cl Chlorine
 Ar Argon
 P Phosphorus
 Ca Calcium
 Sc Scandium
 Ti Titanium
 Cr Chromium
 Mn Manganese
 Fe Iron
 Co Cobalt
 Ni Nickel
 Cu Copper
 Zn Zinc
 Ga Gallium
 Ge Germanium
 As Arsenic
 Se Selenium
 Br Bromine
 Kr Krypton
 Rb Rubidium