Chapter One-Matter, Chemical Trends and Chemical Bonding Flashcards
What is a physical property?
A physical property is a property that you can observe without changing one kind of matter into something new. For example, Iron is a strong metal with a shiny surface, it can be heated to form different shapes, all of these properties can be observed without changing iron into something new.
Complete the following…
Matter is anything that has
mass and volume (takes up space)
What is a chemical property?
A chemical property is a property that you can observe when one kind of matter is converted into a different type of matter. For example, Iron can react with oxygen to form rust, which is a different kind of matter.
What is the difference between a physical and a chemical property?
The difference between a physical and chemical property is that a physical properties can be observed without changing the identity of the substance, while chemical properties can be observed when one kind of matter is converted to another.
Fill in the blank. Physical state, colour, odour, crystal shape, malleability, ductility, hardness and brittleness are all examples of ______________________.
Qualitative Physical Properties
Fill in the blank. Melting point, boiling point, density, solubility, electrical conductivity and thermal conductivity are all examples of ____________________.
Quantitative Physical Properties
Fill in the blank. Reactivity with water, air, dioxide, acids, bases, combustibilty, toxicity and decomposition are all examples of _________________________.
Chemical Properties
Properties of matter using words NOT measurements or numerical data.
Ex. Colour, flammability
Qualitative property
Properties of matter using measurements or numerical data.
Ex. Density, boiling point
Quantitative property
True or False. All non-zero numbers are significant.
Ex. 19.4 = 3 SF
True
True or False. All zeros sandwiched between numbers are significant.
Ex. 408 = 3 SF
True
True or False. Zeros to the left of the first number are significant.
Ex. 0.0907 = 5 SF
False. Zeros to the left of the first number are NOT significant.
Ex. 0.0907 = 3 SF
True or False. Zeros to the right may or may NOT be significant.
Ex. 2000 = 1 SF
2000.0 = 5 SF
True. Decimal adds certainty.
True or False. When adding and subtracting, the fewest number of decimal places in the question is the number you should have in your answer.
True.
True or False. When multiplying and dividing, the greatest number of SFs in the questions is the number you should have in your answer.
False. When multiplying and dividing, the fewest number of SFs in the questions is the number you should have in your answer.
How would you write this number in scientific notation?
0.0000987
9.87x10^-5
How would you write this number in scientific notation?
65000000
6.5x10^7
Is there another way to perform conversions besides the stair method?
Yes, it is possible to use unitary rates. Using a conversion factor (or unitary rate), you can relate or connect two different units.
Define accuracy.
The closeness of a measurement to an accepted value.
Define precison.
The closeness of a measurement to other measurements of thee same object or phenomena.
Fill in the blanks. Matter can be found in three states; _____________, ____________, ______________. Matter is divided into two categories; _______________________ and __________________. In a __________________, matter is only composed of one type of particle and has _________________________________. An ______________ can be composed of a single atom, like Fe. Or composed of 2 or more of the same atoms, like O2. A _______________ is composed of 2 or more elements joined by chemical bonds, like NaCl. In a ___________________, matter is composed of MORE THAN ONE type of particle. A ______________ is a uniform mixture, like salt water. A ________________________ is a non-uniform mixture (with two or more visible components), like muddy water.
A) Solid G) Unique identifiable properties
B) Liquid H) Element
C) Gas I) Compound
D) Pure Substance J) Mixture
E) Mixture K) Solution
F) Pure Substance L) Heterogeneous Mixture
Fill in the blanks. _____________ are the basic substances that make up all matter. The two smallest and least dense of these are _______________ and ____________. Yet, these two account for nearly 98% of the mass of the entire universe!
A) Element
B) Hydrogen
C) Helium
In 1809, John Dalton described atoms as solid, indestructible particles that make up all matter. State his atomic theory.
1) All matter is made us of tiny particles (atoms). An atom cannot be created, destroyed or divided into smaller particles.
2) The atoms of one element cannot be converted into atoms of any other element.
3) All atoms of one element have the same properties, such as mass and size. These properties are different from the properties of the atoms of any other element.
4) Atoms of different elements combine in specific proportions to from compounds.
True or False.
Particle Symbol Mass (u) Charge
Proton p+ 1 1+
Neutron n 1 0
Electron e- 1 /1837 1-
True.
How many _____ are in helium?
Protons?
Electrons?
Neutrons?
4
2 He
Protons = 2
Electrons = 2
Neutrons = 2
Because in scientific notation, the higher number is the mass number, the lower is the atomic number and the letters are the chemical symbol. This is reversed on the periodic table.
True or False. Isotopes are atoms of an element that have the same number of protons and the same number of neutrons.
False. Isotopes are atoms of an element that have the same number of protons but different numbers of neutrons.
How are ions and isotopes related?
Isotopes and ions have varying numbers of sub-atomic particles. Isotopes have varying neutrons while ions have varying electron values. However, the mass of an ion and an isotope will be different and the mass of an ion and an atom will be the same (the mass of electrons is negligilbe).
Fill in the blanks. Some isotopes are more unstable than others. Their nuclei is more likely to decay, releasing energy and subatomic particles in a process called ___________________, which occurs spontaneously. Isotopes that have unstable nuclei are called _____________________.
A) Radioactivity
B) Radioisotopes
What is the difference between and isotope and a radioisotope?
An isotope is natural whereas a radioisotope is spontaneous.
State the Modern Atomic Theory.
1) Although an atom is divisble, it is still the smallest particle of an element that has the properties and identity of the element.
2) Nuclear reactions (changes that alter the composition of the atomic nucleus) may in fact, convert atoms of one element into atoms of another.
3) Different isotopes of an element have different numbers of neutrons and thus different masses. Scientists treat elements as if their atoms have an average mass.
4) Atoms of different elements combine in specific proportions to form compounds.
True or False. Mendeleev sequenced the elements in order of increasing popularity.
False. Mendeleev sequenced the elements in order of increasing atomic mass. Trends began to emerge and this was the creation of the periodic table.
There are ________ main groups of elements.
8
What is one common trend found throughout the main groups on the periodic table?
Main groups have the same number of valence electrons. Group number = number of valence electrons.
Define ionization energy.
The energy that is needed to remove an electron from a neutral atom.
Define valence electron.
An electron that occupies the outermost energy level of an atom.
Define energy level.
Fixed, 3-dimensional volume in which electrons travel around the nucleus.
True or False. Electrons move haphazardly around the nucleus.
False. Their movement is restricted to a fixed region of space called energy shells. An electron moving in a lower energy level is closer to the nucleus.
State the Period-Related Pattern. (row)
An element’s period number is the same as the number of energy levels that the electrons of its atoms occupy.
Ex. period 5 elements have electrons that occupy 5 energy levels.
