Chapter C1- Atomic Structure Flashcards
What are all substances made up of?
What are elements?
What do compounds contain?
What do molecules contain?
What does it mean if a chemical compound contains ate at the end?
What does it mean if the chemical compound contains ide at the end?
What does the law of conservation of mass mean?
What three things are balanced in a chemical equation?
Tiny particles called atoms.
Substances made up of just one type of atom.
Two or more different types of atoms.
More than one atom.
Means it contains oxygen.
Means it contains nothing else (eg potassium chloride).
The law of conservation of mass states that the reactants mass has to equal the products mass in a chemical equation.
Atoms, mass and charge.
What does a nucleus of an atom contain?
What’s an atom made up of?
What are these shells or orbitals?
What is an electrostatic attraction?
Protons and neutrons.
A nucleus containing protons and neutrons, and electrons which travel around the nucleus in shells or orbitals.
These are not actually physical things and don’t physically stay there.
an attraction between a charge of + and -, which holds the electrons close to the nucleus.
What is the charge of a proton?
What is the charge of a neutron?
What is a charge of a electron?
What do electron shells contain?
What does the mass number of an element equal?
What does the atomic number mean and also called?
In an atom, how many protons and electrons are their?
What does this mean concerning the charge of an atom?
+1 (so positive).
0 (so neutral like neutron).
-1 (so negative).
Energy levels.
The mass number equals the number of protons and neutrons added together.
The atomic number (or proton number) means the number of protons in an atom.
In an atom, the number of protons always equals the number of electrons.
This means that an atom is always neutral.
What is an ion?
What does the chemistry of an atom depend on?
What are isotopes?
What do isotopes have?
What is an example of an isotope on the periodic table?
In this example given, what is the mass number called?
Therefore, what do they have that’s different and what do they have that’s always the same?
This is what an atom is called when it gains or loses electrons.
The number of electrons in an atom.
Different forms of the same element.
Isotopes have the same number of protons but a different number of neutrons.
Chlorine (Cl) with a mass number of 35.5.
An average mass.
Isotopes have the same atomic number (or proton number) but a different atomic mass.
What is a substance called that dissolves?
What’s a substance called that won’t dissolve?
What is a solution?
What is the solid and liquid called in a solution?
What is filtration?
What are the substances that stay behind and flow through the filter paper called?
What is evaporation?
What is simple distillation?
What is fractional distillation?
Soluble.
Insoluble.
A solid dissolved in a liquid.
In a solution, the solid is called the solute and the liquid is called the solvent.
Filtration is the method for separating an insoluble solid from a liquid.
The stuff left behind is called the residue and the stuff that flows through is called the filtrate.
Evaporation is used to separate a soluble solid from a liquid.
Simple distillation is a method for separating the solvent from a solution.
Fractional distillation is a method for separating a liquid from a mixture of two or more liquids.
What is chromatography?
What is the structure of electrons for the first 20 elements in the periodic table?
What do chemical bonds involve?
In what two ways can bonds form?
A way of separating different substances that are dissolved in a solution.
First Shell= 2
Second Shell=8 These means the maximum number of electrons per shell.
Third Shell=8
Fourth Shell=2
Involve electrons from the reacting atoms.
- Electrons are transferred from one atom to another, so one atom gives electrons and the other takes electrons.
- Electrons are shared between two atoms.
What happens when the outer electrons have high energy levels?
What does this mean concerning chemical reactions?
What is the relative mass of a proton?
What is the relative mass of a neutron?
What is the relative mass of an electron?
The greater the distance from the nucleus.
The more easily electrons are lost.
1.
1.
Negligible mass (so small that it’s disregarded).
What did John Dalton describe atoms as at the start of the 19th century?
When and what did JJ Thompson do?
In what two ways did he show that atoms must contain even smaller negatively charged particles?
What were these then called?
What was his proposed new theory of atomic structure called?
What did this model show?
What did Ernst Rutherford and student Ernest Marsden conduct and in what year?
How did they do this experiment?
What were they expecting using the plum pudding model as a guide?
Why was this?
What actually happened?
Solid spheres and said that different spheres made up different elements
In 1897, concluded from his experiments that atoms were not just solid spheres
His measurements of charge and mass concluded this
Electrons
The plum pudding model
The atom as a ball of positive charge with electrons stuck in it
In 1909, conducted the alpha particle scattering experiments
By firing positively charged alpha particles at an extremely thin sheet of gold
Expected the particles to pass straight through the sheet or be slightly deflected at most
Because the positive charge of each atom was thought to be very spread out through the “pudding” of the atom
Most of the particles did go straight through the gold sheet, some were deflected more than expected, and a small number were deflected backwards.
What atomic structure model did Rutherford come up with to explain the new evidence after the alpha particles experiment?
Describe this atomic structure model and what does this model propose about the atom?
Using this, what does that mean happened in the alpha particle experiment?
What happened if they were fired directly at the nucleus and what would have otherwise happened?
What did scientists then realised and what would have this caused?
What did Niel Bohr’s nuclear model of the atom suggest?
What did Bohr propose?
What did he propose each shell was?
The nuclear model of an atom
There’s a tiny positively charged nucleus at the centre, where most of the mass is concentrated. A “cloud” of negative electrons surrounds this nucleus meaning that most of the atom is empty space
When the alpha particles came near the concentrated, positive charge of the nucleus they were deflected
They were deflected backwards
Otherwise they passed through the empty space
That electrons in a “cloud” around the nucleus of an atom would be attracted to the nucleus, causing the atom to collapse
That all electrons were contained in shells
That electrons orbit the nucleus in fixed shells that aren’t anywhere in between
In a fixed distance from the nucleus.
What two reason encouraged Bohr’s theory of atomic structure to be accepted?
What did further experiments then show and by who?
What do these particles have and what were they called?
What happened 20 years after scientists had accepted that atoms have nuclei and in what year and by who?
What are these particles now called?
What did the discovery of these particles result in and what is this called?
- It was supported by many experiments
- It helped to explain lots of other scientists’ observations at the time
Further experiments by Rutherford and others showed that the nucleus can be divided into smaller particles
Same charge as a hydrogen nucleus and were called Protons
In 1932, James Chadwick carried out an experiment which provided evidence fro neutral particles in the nucleus
Neutrons
The model of the atom which is pretty close to the modern day accepted version, known as the nuclear model.
